sodium chloride 2NaCl--> 2Na +Cl2 on passing electric current gives sodium and chlorine

The decomposition reaction generally takes place when energy in some form such as heat, electricity or light is supplied to the reactants

When heated CaCO3 s → CO2 g CaO(S)?

decomposition of a substance by heating is thermal decomposition.

Electrolysis: the decomposition of a substance by passing electric current through it is known as electrolysis

sodium chloride 2NaCl--> 2Na +Cl2 on passing electric current gives sodium and chlorine

Photolysis: the decomposition of a compound with light is called photolysis

When heated CaCO3 s → CO2 g CaO(S)?

decomposition of a substance by heating is thermal decomposition.

Electrolysis: the decomposition of a substance by passing electric current through it is known as electrolysis

sodium chloride 2NaCl--> 2Na +Cl2 on passing electric current gives sodium and chlorine

Photolysis: the decomposition of a compound with light is called photolysis

Study of decomposition of silver chloride. Take about 2 grams of silver chloride in a china dish

decomposition of a substance by heating is thermal decomposition.

Electrolysis: the decomposition of a substance by passing electric current through it is known as electrolysis

sodium chloride 2NaCl--> 2Na +Cl2 on passing electric current gives sodium and chlorine

Photolysis: the decomposition of a compound with light is called photolysis

Study of decomposition of silver chloride. Take about 2 grams of silver chloride in a china dish

Place this china dish in the sunlight for some time

Electrolysis: the decomposition of a substance by passing electric current through it is known as electrolysis

sodium chloride 2NaCl--> 2Na +Cl2 on passing electric current gives sodium and chlorine

Photolysis: the decomposition of a compound with light is called photolysis

Study of decomposition of silver chloride. Take about 2 grams of silver chloride in a china dish

Place this china dish in the sunlight for some time

It is observed that the white silver chloride turns gray on exposure to sunlight

When silver chloride is exposed to light, it decomposes to form silver metal and chlorine gas. 2AgCl → 2Ag + Cl2

Photolysis: the decomposition of a compound with light is called photolysis

Study of decomposition of silver chloride. Take about 2 grams of silver chloride in a china dish

Place this china dish in the sunlight for some time

It is observed that the white silver chloride turns gray on exposure to sunlight

When silver chloride is exposed to light, it decomposes to form silver metal and chlorine gas. 2AgCl → 2Ag + Cl2

Silver bromide undergoes decomposition when exposed to light

Study of decomposition of silver chloride. Take about 2 grams of silver chloride in a china dish

Place this china dish in the sunlight for some time

It is observed that the white silver chloride turns gray on exposure to sunlight

When silver chloride is exposed to light, it decomposes to form silver metal and chlorine gas. 2AgCl → 2Ag + Cl2

Silver bromide undergoes decomposition when exposed to light

Silver bromide 2 AgBr → 2 Ag + Br2 when exposed to light gives 2 Ag silver and bromine Br2

Place this china dish in the sunlight for some time

It is observed that the white silver chloride turns gray on exposure to sunlight

When silver chloride is exposed to light, it decomposes to form silver metal and chlorine gas. 2AgCl → 2Ag + Cl2

Silver bromide undergoes decomposition when exposed to light

Silver bromide 2AgBr → 2 Ag + Br2 when exposed to light gives 2 Ag silver and bromine Br2

The above reactions are used in black and white photography

It is observed that the white silver chloride turns gray on exposure to sunlight

When silver chloride is exposed to light, it decomposes to form silver metal and chlorine gas. 2AgCl → 2Ag + Cl2

Silver bromide undergoes decomposition when exposed to light

Silver bromide 2AgBr → 2 Ag + Br2 when exposed to light gives 2 Ag silver and bromine Br2

The above reactions are used in black and white photography

It is observed that the white silver chloride turns gray on exposure to sunlight

When silver chloride is exposed to light, it decomposes to form silver metal and chlorine gas. 2AgCl → 2Ag + Cl2

Silver bromide undergoes decomposition when exposed to light

Silver bromide 2AgBr → 2 Ag + Br2 when exposed to light gives 2 Ag silver and bromine Br2

The above reactions are used in black and white photography

It is observed that the white silver chloride turns gray on exposure to sunlight

When silver chloride is exposed to light, it decomposes to form silver metal and chlorine gas. 2AgCl → 2Ag + Cl2

Silver bromide undergoes decomposition when exposed to light

Silver bromide 2AgBr → 2 Ag + Br2 when exposed to light gives 2 Ag silver and bromine Br2

The above reactions are used in black and white photography

It is observed that the white silver chloride turns gray on exposure to sunlight

When silver chloride is exposed to light, it decomposes to form silver metal and chlorine gas. 2AgCl → 2Ag + Cl2

Silver bromide undergoes decomposition when exposed to light

Silver bromide 2AgBr → 2 Ag + Br2 when exposed to light gives 2 Ag silver and bromine Br2

The above reactions are used in black and white photography

It is observed that the white silver chloride turns gray on exposure to sunlight

Oxidation and reduction redox reaction im formation of copper oxide from copper

Requirement: china dish, copper powder, burner, tripod stand, and wire gauze

Activity: heat a china dish containing some amount of copper powder and observe what will happen?

we can observe the surface of copper powder becoming coated with black copper oxide

because oxygen is added from air to copper and copper oxide is formed 2Cu + O2 ----> 2CuO

Oxidation and reduction redox reaction im formation of copper oxide from copper

Requirement: china dish, copper powder, burner, tripod stand, and wire gauze

Activity: heat a china dish containing some amount of copper powder and observe what will happen?

we can observe the surface of copper powder becoming coated with black copper oxide

because oxygen is added from air to copper and copper oxide is formed 2Cu + O2 ----> 2CuO

If hydrogen gas is passed over this heated material copper oxide; CuO you will the black coating on the surface turns brown

Requirement: china dish, copper powder, burner, tripod stand, and wire gauze

Activity: heat a china dish containing some amount of copper powder and observe what will happen?

we can observe the surface of copper powder becoming coated with black copper oxide

because oxygen is added from air to copper and copper oxide is formed 2Cu + O2 ----> 2CuO

If hydrogen gas is passed over this heated material copper oxide; CuO you will the black coating on the surface turns brown

due to reverse reaction and copper is obtained CuO + H2 → Cu + H2O

Activity: heat a china dish containing some amount of copper powder and observe what will happen?

we can observe the surface of copper powder becoming coated with black copper oxide

because oxygen is added from air to copper and copper oxide is formed 2Cu + O2 ----> 2CuO

If hydrogen gas is passed over this heated material copper oxide; CuO you will the black coating on the surface turns brown

due to reverse reaction and copper is obtained CuO + H2 → Cu + H2O

if substance gains oxygen during a reaction is called oxidized

we can observe the surface of copper powder becoming coated with black copper oxide

because oxygen is added from air to copper and copper oxide is formed 2Cu + O2 ----> 2CuO

If hydrogen gas is passed over this heated material copper oxide; CuO you will the black coating on the surface turns brown

due to reverse reaction and copper is obtained CuO + H2 → Cu + H2O

if substance gains oxygen during a reaction is called oxidized

we can observe the surface of copper powder becoming coated with black copper oxide

because oxygen is added from air to copper and copper oxide is formed 2Cu + O2 ----> 2CuO

If hydrogen gas is passed over this heated material copper oxide; CuO you will the black coating on the surface turns brown

due to reverse reaction and copper is obtained CuO + H2 → Cu + H2O

if substance gains oxygen during a reaction is called oxidized

if substance loses oxygen during the reaction is called reduced

because oxygen is added from air to copper and copper oxide is formed 2Cu + O2 ----> 2CuO

If hydrogen gas is passed over this heated material copper oxide; CuO you will the black coating on the surface turns brown

due to reverse reaction and copper is obtained CuO + H2 → Cu + H2O

if substance gains oxygen during a reaction is called oxidized

if substance loses oxygen during the reaction is called reduced

because oxygen is added from air to copper and copper oxide is formed 2Cu + O2 ----> 2CuO

If hydrogen gas is passed over this heated material copper oxide; CuO you will the black coating on the surface turns brown

due to reverse reaction and copper is obtained CuO + H2 → Cu + H2O

if substance gains oxygen during a reaction is called oxidized

if substance loses oxygen during the reaction is called reduced

in this reaction copper II oxide is losing oxygen and is being reduced

the hydrogen is gaining oxygen and is being oxidized

due to reverse reaction and copper is obtained CuO + H2 → Cu + H2O

if substance gains oxygen during a reaction is called oxidized

if substance loses oxygen during the reaction is called reduced

in this reaction copper II oxide is losing oxygen and is being reduced

the hydrogen is gaining oxygen and is being oxidized

One reactant gets oxidized while the other gets reduced during reaction is called redox reaction

if substance gains oxygen during a reaction is called oxidized

if substance loses oxygen during the reaction is called reduced

in this reaction copper II oxide is losing oxygen and is being reduced

the hydrogen is gaining oxygen and is being oxidized

One reactant gets oxidized while the other gets reduced during reaction is called redox reaction

if substance gains oxygen during a reaction is called oxidized

if substance loses oxygen during the reaction is called reduced

in this reaction copper II oxide is losing oxygen and is being reduced

the hydrogen is gaining oxygen and is being oxidized

One reactant gets oxidized while the other gets reduced during reaction is called redox reaction

if substance gains oxygen during a reaction is called oxidized

if substance loses oxygen during the reaction is called reduced

in this reaction copper II oxide is losing oxygen and is being reduced

the hydrogen is gaining oxygen and is being oxidized

One reactant gets oxidized while the other gets reduced during reaction is called redox reaction

if substance gains oxygen during a reaction is called oxidized

if substance loses oxygen during the reaction is called reduced

in this reaction copper II oxide is losing oxygen and is being reduced

the hydrogen is gaining oxygen and is being oxidized

One reactant gets oxidized while the other gets reduced during reaction is called redox reaction

if substance gains oxygen during a reaction is called oxidized

if substance loses oxygen during the reaction is called reduced

in this reaction copper II oxide is losing oxygen and is being reduced

Relative Reactivity of Metals Zinc. Take about 20 ml of 1M solution of copper sulphate, aluminium sulphate and ferrous sulphate

in three different beakers, and some zinc metal pieces in a watch glass.

Take some zinc metal pieces using forceps. Using a forceps add 2 pieces of zinc into the beakers containing ferrous sulphate, aluminium

sulphate and copper sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions and the appearance of the metal.

In the beaker containing of copper sulphate solution, the blue colour of copper sulphate disappears and red-brown particles of copper settles down at the bottom of the beaker.

This indicates that Zn is more reactive than Cu and it can displace Cu from CuSO4 solution

and form colourless solution of ZnSO4.

In the case of aluminium sulphate solution, no change is observed.

Take some zinc metal pieces using forceps. Using a forceps add 2 pieces of zinc into the beakers containing ferrous sulphate, aluminium

sulphate and copper sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions and the appearance of the metal.

In the beaker containing of copper sulphate solution, the blue colour of copper sulphate disappears and red-brown particles of copper settles down at the bottom of the beaker.

This indicates that Zn is more reactive than Cu and it can displace Cu from CuSO4 solution

and form colourless solution of ZnSO4.

In the case of aluminium sulphate solution, no change is observed.

Because Zn is less reactive than Al so it cannot displace Al from Al2(SO4)3 solution.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions and the appearance of the metal.

In the beaker containing of copper sulphate solution, the blue colour of copper sulphate disappears and red-brown particles of copper settles down at the bottom of the beaker.

This indicates that Zn is more reactive than Cu and it can displace Cu from CuSO4 solution

and form colourless solution of ZnSO4.

In the case of aluminium sulphate solution, no change is observed.

Because Zn is less reactive than Al so it cannot displace Al from Al2(SO4)3 solution.

In the case of ferrous sulphate solution, the green colour of ferrous sulphate disappears

and iron particles settle down at the bottom of the beaker.

In the beaker containing of copper sulphate solution, the blue colour of copper sulphate disappears and red-brown particles of copper settles down at the bottom of the beaker.

This indicates that Zn is more reactive than Cu and it can displace Cu from CuSO4 solution

and form colourless solution of ZnSO4.

In the case of aluminium sulphate solution, no change is observed.

Because Zn is less reactive than Al so it cannot displace Al from Al2(SO4)3 solution.

In the case of ferrous sulphate solution, the green colour of ferrous sulphate disappears

and iron particles settle down at the bottom of the beaker.

This indicates that Zn is more reactive than Fe and it can displace Fe from FeSO4 solution

and form a colourless solution of ZnSO4.

This indicates that Zn is more reactive than Cu and it can displace Cu from CuSO4 solution

and form colourless solution of ZnSO4.

In the case of aluminium sulphate solution, no change is observed.

Because Zn is less reactive than Al so it cannot displace Al from Al2(SO4)3 solution.

In the case of ferrous sulphate solution, the green colour of ferrous sulphate disappears

and iron particles settle down at the bottom of the beaker.

This indicates that Zn is more reactive than Fe and it can displace Fe from FeSO4 solution

and form a colourless solution of ZnSO4.

Copper Take about 20ml of zinc sulphate, aluminium sulphate and ferrous sulphate solutions in three different beakers, and some copper metal

pieces in a watch glass.

Using a forceps add 2 pieces of copper into the beaker containing ferrous sulphate, aluminium

sulphate and zinc sulphate solutions.

Because Zn is less reactive than Al so it cannot displace Al from Al2(SO4)3 solution.

In the case of ferrous sulphate solution, the green colour of ferrous sulphate disappears

and iron particles settle down at the bottom of the beaker.

This indicates that Zn is more reactive than Fe and it can displace Fe from FeSO4 solution

and form a colourless solution of ZnSO4.

Copper Take about 20ml of zinc sulphate, aluminium sulphate and ferrous sulphate solutions in three different beakers, and some copper metal

pieces in a watch glass.

Using a forceps add 2 pieces of copper into the beaker containing ferrous sulphate, aluminium

sulphate and zinc sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions

and the appearance of the metal.

In the case of ferrous sulphate solution, the green colour of ferrous sulphate disappears

and iron particles settle down at the bottom of the beaker.

This indicates that Zn is more reactive than Fe and it can displace Fe from FeSO4 solution

and form a colourless solution of ZnSO4.

Copper Take about 20ml of zinc sulphate, aluminium sulphate and ferrous sulphate solutions in three different beakers, and some copper metal

pieces in a watch glass.

Using a forceps add 2 pieces of copper into the beaker containing ferrous sulphate, aluminium

sulphate and zinc sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions

and the appearance of the metal.

In the case of ferrous sulphate solution, the green colour of ferrous sulphate disappears

and iron particles settle down at the bottom of the beaker.

This indicates that Zn is more reactive than Fe and it can displace Fe from FeSO4 solution

and form a colourless solution of ZnSO4.

Copper Take about 20ml of zinc sulphate, aluminium sulphate and ferrous sulphate solutions in three different beakers, and some copper metal

pieces in a watch glass.

Using a forceps add 2 pieces of copper into the beaker containing ferrous sulphate, aluminium

sulphate and zinc sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions

and the appearance of the metal.

There is no change in the colour of the three salt solutions as well as the appearance of

the metal pieces.

This indicates that Zn is more reactive than Fe and it can displace Fe from FeSO4 solution

and form a colourless solution of ZnSO4.

Copper Take about 20ml of zinc sulphate, aluminium sulphate and ferrous sulphate solutions in three different beakers, and some copper metal

pieces in a watch glass.

Using a forceps add 2 pieces of copper into the beaker containing ferrous sulphate, aluminium

sulphate and zinc sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions

and the appearance of the metal.

There is no change in the colour of the three salt solutions as well as the appearance of

the metal pieces.

This reaction indicates that Cu is less reactive than the other three metals Al, Zn and Fe

so it cannot displace these metals from their salt solutions.

Aluminium Take about 20ml of copper sulphate, zinc sulpahte

and ferrous sulphate solutions in three different beakers, and some aluminium metal pieces in

a watch glass.

Using a forceps add 2 pieces of copper into the beaker containing ferrous sulphate, aluminium

sulphate and zinc sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions

and the appearance of the metal.

There is no change in the colour of the three salt solutions as well as the appearance of

the metal pieces.

This reaction indicates that Cu is less reactive than the other three metals Al, Zn and Fe

so it cannot displace these metals from their salt solutions.

Copper Take about 20ml of zinc sulphate, aluminium sulphate and ferrous sulphate solutions in three different beakers, and some copper metal

pieces in a watch glass.

Using a forceps add 2 piece of aluminium into the beaker containing ferrous sulphate, zinc sulphate and copper sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions

and the appearance of the metal.

There is no change in the colour of the three salt solutions as well as the appearance of

the metal pieces.

This reaction indicates that Cu is less reactive than the other three metals Al, Zn and Fe

so it cannot displace these metals from their salt solutions.

Aluminium Take about 20ml of copper sulphate, zinc sulpahte

and ferrous sulphate solutions in three different beakers, and some aluminium metal pieces in

a watch glass.

Using a forceps add 2 piece of aluminium into the beaker containing ferrous sulphate, zinc sulphate and copper sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions

and the appearance of the metal.

There is no change in the colour of the three salt solutions as well as the appearance of

the metal pieces.

This reaction indicates that Cu is less reactive than the other three metals Al, Zn and Fe

so it cannot displace these metals from their salt solutions.

Aluminium Take about 20ml of copper sulphate, zinc sulpahte

and ferrous sulphate solutions in three different beakers, and some aluminium metal pieces in

a watch glass.

Using a forceps add 2 piece of aluminium into the beaker containing ferrous sulphate, zinc sulphate and copper sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions

and the appearance of the metal.

In the case of copper sulphate solution, the blue colour of copper sulphate disappears

and red-brown particles of copper settle down at the bottom of the beaker.

This reaction indicates that Cu is less reactive than the other three metals Al, Zn and Fe

so it cannot displace these metals from their salt solutions.

Aluminium Take about 20ml of copper sulphate, zinc sulpahte

and ferrous sulphate solutions in three different beakers, and some aluminium metal pieces in

a watch glass.

Using a forceps add 2 piece of aluminium into the beaker containing ferrous sulphate, zinc sulphate and copper sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions

and the appearance of the metal.

In the case of copper sulphate solution, the blue colour of copper sulphate disappears

and red-brown particles of copper settle down at the bottom of the beaker.

This indicates that Al is more reactive than Cu and it can displace Cu from CuSO4 solution

and form a colourless solution of Al2(SO4)3.

Aluminium Take about 20ml of copper sulphate, zinc sulpahte

and ferrous sulphate solutions in three different beakers, and some aluminium metal pieces in

a watch glass.

Using a forceps add 2 piece of aluminium into the beaker containing ferrous sulphate, zinc sulphate and copper sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions

and the appearance of the metal.

In the case of copper sulphate solution, the blue colour of copper sulphate disappears

and red-brown particles of copper settle down at the bottom of the beaker.

This indicates that Al is more reactive than Cu and it can displace Cu from CuSO4 solution

and form a colourless solution of Al2(SO4)3.

In the case of zinc sulphate solution, the solution remains colourless and Zn particles

settle down at the bottom of the beaker.

This indicates that Al is more reactive than Zn and it can displace Zn from ZnSO4 solution

and form a colourless solution of Al2(SO4)3.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions

and the appearance of the metal.

In the case of copper sulphate solution, the blue colour of copper sulphate disappears

and red-brown particles of copper settle down at the bottom of the beaker.

This indicates that Al is more reactive than Cu and it can displace Cu from CuSO4 solution

and form a colourless solution of Al2(SO4)3.

In the case of zinc sulphate solution, the solution remains colourless and Zn particles

settle down at the bottom of the beaker.

This indicates that Al is more reactive than Zn and it can displace Zn from ZnSO4 solution

and form a colourless solution of Al2(SO4)3.

In the case of ferrous sulphate solution, the green colour of ferrous sulphate disappears

and iron particles settle down at the bottom of the beaker.

In the case of copper sulphate solution, the blue colour of copper sulphate disappears

and red-brown particles of copper settle down at the bottom of the beaker.

This indicates that Al is more reactive than Cu and it can displace Cu from CuSO4 solution

and form a colourless solution of Al2(SO4)3.

In the case of zinc sulphate solution, the solution remains colourless and Zn particles

settle down at the bottom of the beaker.

This indicates that Al is more reactive than Zn and it can displace Zn from ZnSO4 solution

and form a colourless solution of Al2(SO4)3.

In the case of ferrous sulphate solution, the green colour of ferrous sulphate disappears

and iron particles settle down at the bottom of the beaker.

This indicates that Al is more reactive than Fe and it can displace Fe from FeSO4 solution

and form a colourless solution of Al2(SO4)3.

This indicates that Al is more reactive than Cu and it can displace Cu from CuSO4 solution

and form a colourless solution of Al2(SO4)3.

In the case of zinc sulphate solution, the solution remains colourless and Zn particles

settle down at the bottom of the beaker.

This indicates that Al is more reactive than Zn and it can displace Zn from ZnSO4 solution

and form a colourless solution of Al2(SO4)3.

In the case of ferrous sulphate solution, the green colour of ferrous sulphate disappears

and iron particles settle down at the bottom of the beaker.

This indicates that Al is more reactive than Fe and it can displace Fe from FeSO4 solution

and form a colourless solution of Al2(SO4)3.

Iron: Take about 20ml of copper sulpahte, zinc sulphate

and aluminium sulpahte solutions in three different beakers, and some iron metal pieces

in a watch glass.

In the case of zinc sulphate solution, the solution remains colourless and Zn particles

settle down at the bottom of the beaker.

This indicates that Al is more reactive than Zn and it can displace Zn from ZnSO4 solution

and form a colourless solution of Al2(SO4)3.

In the case of ferrous sulphate solution, the green colour of ferrous sulphate disappears

and iron particles settle down at the bottom of the beaker.

This indicates that Al is more reactive than Fe and it can displace Fe from FeSO4 solution

and form a colourless solution of Al2(SO4)3.

Iron: Take about 20ml of copper sulpahte, zinc sulphate

and aluminium sulpahte solutions in three different beakers, and some iron metal pieces

in a watch glass.

Using a forceps add 2 piece of iron into the beakers containing aluminium sulphate, zinc sulphate and copper sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions and the appearance of the metal.

In the case of ferrous sulphate solution, the green colour of ferrous sulphate disappears

and iron particles settle down at the bottom of the beaker.

This indicates that Al is more reactive than Fe and it can displace Fe from FeSO4 solution

and form a colourless solution of Al2(SO4)3.

Iron: Take about 20ml of copper sulpahte, zinc sulphate

and aluminium sulpahte solutions in three different beakers, and some iron metal pieces

in a watch glass.

Using a forceps add 2 piece of iron into the beakers containing aluminium sulphate, zinc sulphate and copper sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions and the appearance of the metal.

In the case of copper sulphate solution, the blue colour of copper sulphate changes to light green and red-brown particles of copper settle down at the bottom of the beaker.

This indicates that Al is more reactive than Fe and it can displace Fe from FeSO4 solution

and form a colourless solution of Al2(SO4)3.

Iron: Take about 20ml of copper sulpahte, zinc sulphate

and aluminium sulpahte solutions in three different beakers, and some iron metal pieces

in a watch glass.

Using a forceps add 2 piece of iron into the beakers containing aluminium sulphate, zinc sulphate and copper sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions and the appearance of the metal.

In the case of copper sulphate solution, the blue colour of copper sulphate changes to light green and red-brown particles of copper settle down at the bottom of the beaker.

This indicates that Fe is more reactive than Cu and it can displace Cu from CuSO4 solution and form a light green coloured FeSO4 solution.

Iron: Take about 20ml of copper sulpahte, zinc sulphate

and aluminium sulpahte solutions in three different beakers, and some iron metal pieces

in a watch glass.

Using a forceps add 2 piece of iron into the beakers containing aluminium sulphate, zinc sulphate and copper sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions and the appearance of the metal.

In the case of copper sulphate solution, the blue colour of copper sulphate changes to light green and red-brown particles of copper settle down at the bottom of the beaker.

This indicates that Fe is more reactive than Cu and it can displace Cu from CuSO4 solution and form a light green coloured FeSO4 solution.

In the other two cases, there is no change in the colour of the solution as well as the appearance of the metal pieces.

Using a forceps add 2 piece of iron into the beakers containing aluminium sulphate, zinc sulphate and copper sulphate solutions.

Leave the beakers undisturbed for 1 hour and note the changes in colour of the solutions and the appearance of the metal.

In the case of copper sulphate solution, the blue colour of copper sulphate changes to light green and red-brown particles of copper settle down at the bottom of the beaker.

This indicates that Fe is more reactive than Cu and it can displace Cu from CuSO4 solution and form a light green coloured FeSO4 solution.

In the other two cases, there is no change in the colour of the solution as well as the appearance of the metal pieces.

This indicates that Fe is less reactive than the other two metals Al and Zn so it cannot displace these metals from their salt solutions.

Order of reactivity From these reactions we can infer that Fe is able to displace Cu from its salt solution, Zn is able to displace Cu and Fe from their

salt solutions and Al is able to displace Zn from its salt solution.

In the case of copper sulphate solution, the blue colour of copper sulphate changes to light green and red-brown particles of copper settle down at the bottom of the beaker.

This indicates that Fe is more reactive than Cu and it can displace Cu from CuSO4 solution and form a light green coloured FeSO4 solution.

In the other two cases, there is no change in the colour of the solution as well as the appearance of the metal pieces.

This indicates that Fe is less reactive than the other two metals Al and Zn so it cannot displace these metals from their salt solutions.

Order of reactivity From these reactions we can infer that Fe is able to displace Cu from its salt solution, Zn is able to displace Cu and Fe from their

salt solutions and Al is able to displace Zn from its salt solution.

So Al is the most reactive metal and copper is the least reactive metal.

This indicates that Fe is more reactive than Cu and it can displace Cu from CuSO4 solution and form a light green coloured FeSO4 solution.

In the other two cases, there is no change in the colour of the solution as well as the appearance of the metal pieces.

This indicates that Fe is less reactive than the other two metals Al and Zn so it cannot displace these metals from their salt solutions.

Order of reactivity From these reactions we can infer that Fe is able to displace Cu from its salt solution, Zn is able to displace Cu and Fe from their

salt solutions and Al is able to displace Zn from its salt solution.

So Al is the most reactive metal and copper is the least reactive metal.

This indicates that Fe is more reactive than Cu and it can displace Cu from CuSO4 solution and form a light green coloured FeSO4 solution.

In the other two cases, there is no change in the colour of the solution as well as the appearance of the metal pieces.

This indicates that Fe is less reactive than the other two metals Al and Zn so it cannot displace these metals from their salt solutions.

Order of reactivity From these reactions we can infer that Fe is able to displace Cu from its salt solution, Zn is able to displace Cu and Fe from their

salt solutions and Al is able to displace Zn from its salt solution.

So Al is the most reactive metal and copper is the least reactive metal.

This indicates that Fe is more reactive than Cu and it can displace Cu from CuSO4 solution and form a light green coloured FeSO4 solution.

In the other two cases, there is no change in the colour of the solution as well as the appearance of the metal pieces.

This indicates that Fe is less reactive than the other two metals Al and Zn so it cannot displace these metals from their salt solutions.

Order of reactivity From these reactions we can infer that Fe is able to displace Cu from its salt solution, Zn is able to displace Cu and Fe from their

salt solutions and Al is able to displace Zn from its salt solution.

So Al is the most reactive metal and copper is the least reactive metal.

This indicates that Fe is more reactive than Cu and it can displace Cu from CuSO4 solution and form a light green coloured FeSO4 solution.

In the other two cases, there is no change in the colour of the solution as well as the appearance of the metal pieces.

This indicates that Fe is less reactive than the other two metals Al and Zn so it cannot displace these metals from their salt solutions.

Order of reactivity From these reactions we can infer that Fe is able to displace Cu from its salt solution, Zn is able to displace Cu and Fe from their

salt solutions and Al is able to displace Zn from its salt solution.

So Al is the most reactive metal and copper is the least reactive metal.

This indicates that Fe is more reactive than Cu and it can displace Cu from CuSO4 solution and form a light green coloured FeSO4 solution.

In the other two cases, there is no change in the colour of the solution as well as the appearance of the metal pieces.

This indicates that Fe is less reactive than the other two metals Al and Zn so it cannot displace these metals from their salt solutions.

yes

no

Not enough information

Left side is balanced

4, 5

1, 6

3, 8

2,2

2, 6, 3, 2

it is already balanced

4, 12, 3, 4

2, 1, 4, 5

3,1,2

1,1,1

1,3,1

2,6,3

3,1,3,1

1,3,3,1

1,1,1,3

1,3,1,3

PbO₂ + 2H₂--> H₂SO₄

SO₂ + H₂0 --> H₂SO₄

2Na + 2H₂O --> 2NaOH + H₂

2Na + 2H₂O --> 2NaOH + H

2,3,3,2

2,3,2,3

4,6,6,2

1,3,3,1

1,1,2

1,3,3

3,2,1

1,3,2

K, Na, Ba, Ca, Zn

Mg, Al, Zn, Fe, Ar

Cl, Br, K, Hg, Au

H, C, O, N, P

salt + water

water + hydrogen

salt + hydrogen

salt

Na^-

Na⁺

Na²⁺

Na^2-

Cl⁺

Cl²⁺

Cl^-

Cl^2-

1,2,2,2

2,1,2,2

2,2,1,2

2,2,2,1

Na + HNO3 => NaNO3 + H2

2Na + HNO3 => NaNO3 + H2

2Na + 2HNO3 => NaNO3 + H2

2Na + 2HNO3 => 2NaNO3 + H2

This lesson looks at what happens when brine Undergoes electrolysis

you may need to look at our lesson what happens in electrolysis before going any further.

the electrolysis of brine is an industrial process which is carried out on a large scale but we can look at the process on a smaller scale

in the laboratory brine is a saturated solution of sodium chloride.

we don't want the electrode to become part of this reaction and so we use carbon electrodes.

from the sodium chloride we have positive sodium ions na+ and negative chloride ions cl-

you may need to look at our lesson what happens in electrolysis before going any further.

the electrolysis of brine is an industrial process which is carried out on a large scale but we can look at the process on a smaller scale

in the laboratory brine is a saturated solution of sodium chloride.

we don't want the electrode to become part of this reaction and so we use carbon electrodes.

from the sodium chloride we have positive sodium ions na+ and negative chloride ions cl-

and from the water we have positive hydrogen ions h plus and negative hydroxide ions o h minus

the electrolysis of brine is an industrial process which is carried out on a large scale but we can look at the process on a smaller scale

in the laboratory brine is a saturated solution of sodium chloride.

we don't want the electrode to become part of this reaction and so we use carbon electrodes.

from the sodium chloride we have positive sodium ions na+ and negative chloride ions cl-

and from the water we have positive hydrogen ions h plus and negative hydroxide ions o h minus

when the current flows you will begin to see tiny bubbles of gas forming at each electrode both hydrogen and chlorine gas

are formed

in the laboratory brine is a saturated solution of sodium chloride.

we don't want the electrode to become part of this reaction and so we use carbon electrodes.

from the sodium chloride we have positive sodium ions na+ and negative chloride ions cl-

and from the water we have positive hydrogen ions h plus and negative hydroxide ions o h minus

when the current flows you will begin to see tiny bubbles of gas forming at each electrode both hydrogen and chlorine gas

are formed

but can you work out which electrode produces which gas pause the video and see if you can work it out

we don't want the electrode to become part of this reaction and so we use carbon electrodes.

from the sodium chloride we have positive sodium ions na+ and negative chloride ions cl-

and from the water we have positive hydrogen ions h plus and negative hydroxide ions o h minus

when the current flows you will begin to see tiny bubbles of gas forming at each electrode both hydrogen and chlorine gas

are formed

but can you work out which electrode produces which gas pause the video and see if you can work it out

the chlorine is formed at the anode that's the positive electrode

and hydrogen is formed at the cathode that's the negative electrode

and from the water we have positive hydrogen ions h plus and negative hydroxide ions o h minus

when the current flows you will begin to see tiny bubbles of gas forming at each electrode both hydrogen and chlorine gas

are formed

but can you work out which electrode produces which gas pause the video and see if you can work it out

the chlorine is formed at the anode that's the positive electrode

and hydrogen is formed at the cathode that's the negative electrode

and from the water we have positive hydrogen ions h plus and negative hydroxide ions o h minus

when the current flows you will begin to see tiny bubbles of gas forming at each electrode both hydrogen and chlorine gas

are formed

but can you work out which electrode produces which gas pause the video and see if you can work it out

the chlorine is formed at the anode that's the positive electrode

and hydrogen is formed at the cathode that's the negative electrode

did you get it right let's look at what's going on at each

electrode

when the current flows you will begin to see tiny bubbles of gas forming at each electrode both hydrogen and chlorine gas

are formed

but can you work out which electrode produces which gas pause the video and see if you can work it out

the chlorine is formed at the anode that's the positive electrode

and hydrogen is formed at the cathode that's the negative electrode

did you get it right let's look at what's going on at each

electrode

the anode is positive and attracts the negative chloride and

hydroxide ions

but can you work out which electrode produces which gas pause the video and see if you can work it out

the chlorine is formed at the anode that's the positive electrode

and hydrogen is formed at the cathode that's the negative electrode

did you get it right let's look at what's going on at each

electrode

the anode is positive and attracts the negative chloride and

hydroxide ions

the chloride ions give up their electrons to the anode and are

oxidized to chlorine molecules

the chlorine is formed at the anode that's the positive electrode

and hydrogen is formed at the cathode that's the negative electrode

did you get it right let's look at what's going on at each

electrode

the anode is positive and attracts the negative chloride and

hydroxide ions

the chloride ions give up their electrons to the anode and are

oxidized to chlorine molecules

two ions need to be oxidized to make a diatomic chlorine molecule and two free electrons are produced

the electrons are given up to the anode and the chlorine gas

bubbles up to the surface of the cell

did you get it right let's look at what's going on at each

electrode

the anode is positive and attracts the negative chloride and

hydroxide ions

the chloride ions give up their electrons to the anode and are

oxidized to chlorine molecules

two ions need to be oxidized to make a diatomic chlorine molecule and two free electrons are produced

the electrons are given up to the anode and the chlorine gas

bubbles up to the surface of the cell

if you collected the gas from the anode in a test

tube then you would be able to see the pale green color of the chlorine gas

it will turn down blue litmus paper red showing that it is acidic and then it bleaches it well

the anode is positive and attracts the negative chloride and

hydroxide ions

the chloride ions give up their electrons to the anode and are

oxidized to chlorine molecules

two ions need to be oxidized to make a diatomic chlorine molecule and two free electrons are produced

the electrons are given up to the anode and the chlorine gas

bubbles up to the surface of the cell

if you collected the gas from the anode in a test

tube then you would be able to see the pale green color of the chlorine gas

it will turn down blue litmus paper red showing that it is acidic and then it bleaches it well

what about the cathode? it is negatively charged and attracts the positive sodium and the hydrogen ions

the chloride ions give up their electrons to the anode and are

oxidized to chlorine molecules

two ions need to be oxidized to make a diatomic chlorine molecule and two free electrons are produced

the electrons are given up to the anode and the chlorine gas

bubbles up to the surface of the cell

if you collected the gas from the anode in a test

tube then you would be able to see the pale green color of the chlorine gas

it will turn down blue litmus paper red showing that it is acidic and then it bleaches it well

what about the cathode? it is negatively charged and attracts the positive sodium and the hydrogen ions

the hydrogen ions each gain an electron from the electrode to

form hydrogen atoms

two ions need to be oxidized to make a diatomic chlorine molecule and two free electrons are produced

the electrons are given up to the anode and the chlorine gas

bubbles up to the surface of the cell

if you collected the gas from the anode in a test

tube then you would be able to see the pale green color of the chlorine gas

it will turn down blue litmus paper red showing that it is acidic and then it bleaches it well

what about the cathode? it is negatively charged and attracts the positive sodium and the hydrogen ions

the hydrogen ions each gain an electron from the electrode to

form hydrogen atoms

here's the equation two hydrogen atoms then bond to form a diatomic hydrogen molecule and that's the hydrogen gas given off

the gas here is colourless and can be collected in a test tube

the test to prove that it is hydrogen is done with a burning wooden splint and you'll hear a familiar pop as the hydrogen burns

if you collected the gas from the anode in a test

tube then you would be able to see the pale green color of the chlorine gas

it will turn down blue litmus paper red showing that it is acidic and then it bleaches it well

what about the cathode? it is negatively charged and attracts the positive sodium and the hydrogen ions

the hydrogen ions each gain an electron from the electrode to

form hydrogen atoms

here's the equation two hydrogen atoms then bond to form a diatomic hydrogen molecule and that's the hydrogen gas given off

the gas here is colourless and can be collected in a test tube

the test to prove that it is hydrogen is done with a burning wooden splint and you'll hear a familiar pop as the hydrogen burns

the ions left in the solution are the positive sodium ions and the negative hydroxide ions which combine to form sodium hydroxide

what about the cathode? it is negatively charged and attracts the positive sodium and the hydrogen ions

the hydrogen ions each gain an electron from the electrode to

form hydrogen atoms

here's the equation two hydrogen atoms then bond to form a diatomic hydrogen molecule and that's the hydrogen gas given off

the gas here is colourless and can be collected in a test tube

the test to prove that it is hydrogen is done with a burning wooden splint and you'll hear a familiar pop as the hydrogen burns

the ions left in the solution are the positive sodium ions and the negative hydroxide ions which combine to form sodium hydroxide

overall the electrolysis of brine has produced hydrogen chlorine and sodium hydroxide

the hydrogen ions each gain an electron from the electrode to

form hydrogen atoms

here's the equation two hydrogen atoms then bond to form a diatomic hydrogen molecule and that's the hydrogen gas given off

the gas here is colourless and can be collected in a test tube

the test to prove that it is hydrogen is done with a burning wooden splint and you'll hear a familiar pop as the hydrogen burns

the ions left in the solution are the positive sodium ions and the negative hydroxide ions which combine to form sodium hydroxide

overall the electrolysis of brine has produced hydrogen chlorine and sodium hydroxide

and so we can write a summary equation concentrated sodium chloride solution plus water when electrolyzed gives sodium hydroxide solution hydrogen gas and chlorine gas

2NaCl + 2H2H2O →→ 2NaOH + H2H2 + Cl2Cl2

here's the equation two hydrogen atoms then bond to form a diatomic hydrogen molecule and that's the hydrogen gas given off

the gas here is colourless and can be collected in a test tube

the test to prove that it is hydrogen is done with a burning wooden splint and you'll hear a familiar pop as the hydrogen burns

the ions left in the solution are the positive sodium ions and the negative hydroxide ions which combine to form sodium hydroxide

overall the electrolysis of brine has produced hydrogen chlorine and sodium hydroxide

and so we can write a summary equation concentrated sodium chloride solution plus water when electrolyzed gives sodium hydroxide solution hydrogen gas and chlorine gas

2NaCl + 2H2H2O →→ 2NaOH + H2H2 + Cl2Cl2

here's the equation two hydrogen atoms then bond to form a diatomic hydrogen molecule and that's the hydrogen gas given off

the gas here is colourless and can be collected in a test tube

the test to prove that it is hydrogen is done with a burning wooden splint and you'll hear a familiar pop as the hydrogen burns

the ions left in the solution are the positive sodium ions and the negative hydroxide ions which combine to form sodium hydroxide

overall the electrolysis of brine has produced hydrogen chlorine and sodium hydroxide

and so we can write a summary equation concentrated sodium chloride solution plus water when electrolyzed gives sodium hydroxide solution hydrogen gas and chlorine gas

2NaCl + 2H2H2O →→ 2NaOH + H2H2 + Cl2Cl2

these products are very useful and the electrolysis of brine is done on a much larger industrial scale

chlorine is used to kill bacteria and it is soluble in water

if you've ever visited a public swimming pool then you'll be familiar with the smell of chlorinated water and it's also

used to sterilize water in the main water supply

the ions left in the solution are the positive sodium ions and the negative hydroxide ions which combine to form sodium hydroxide

overall the electrolysis of brine has produced hydrogen chlorine and sodium hydroxide

and so we can write a summary equation concentrated sodium chloride solution plus water when electrolyzed gives sodium hydroxide solution hydrogen gas and chlorine gas

2NaCl + 2H2H2O →→ 2NaOH + H2H2 + Cl2Cl2

these products are very useful and the electrolysis of brine is done on a much larger industrial scale

chlorine is used to kill bacteria and it is soluble in water

if you've ever visited a public swimming pool then you'll be familiar with the smell of chlorinated water and it's also

used to sterilize water in the main water supply

what's more chlorine is one of the main ingredients of bleach which is used in a lot of cleaning products

overall the electrolysis of brine has produced hydrogen chlorine and sodium hydroxide

and so we can write a summary equation concentrated sodium chloride solution plus water when electrolyzed gives sodium hydroxide solution hydrogen gas and chlorine gas

2NaCl + 2H2H2O →→ 2NaOH + H2H2 + Cl2Cl2

these products are very useful and the electrolysis of brine is done on a much larger industrial scale

chlorine is used to kill bacteria and it is soluble in water

if you've ever visited a public swimming pool then you'll be familiar with the smell of chlorinated water and it's also

used to sterilize water in the main water supply

what's more chlorine is one of the main ingredients of bleach which is used in a lot of cleaning products

but this is only scratching the tip of the iceberg as chlorine is used to make dry cleaning ingredients electrical insulators

building materials, refrigerator gasses weed killer pesticides

and is some of the hydrogen and chlorine from the industrial process is combined to form hydrogen chloride gas

and so we can write a summary equation concentrated sodium chloride solution plus water when electrolyzed gives sodium hydroxide solution hydrogen gas and chlorine gas

2NaCl + 2H2H2O →→ 2NaOH + H2H2 + Cl2Cl2

these products are very useful and the electrolysis of brine is done on a much larger industrial scale

chlorine is used to kill bacteria and it is soluble in water

if you've ever visited a public swimming pool then you'll be familiar with the smell of chlorinated water and it's also

used to sterilize water in the main water supply

what's more chlorine is one of the main ingredients of bleach which is used in a lot of cleaning products

but this is only scratching the tip of the iceberg as chlorine is used to make dry cleaning ingredients electrical insulators

building materials, refrigerator gasses weed killer pesticides

and is some of the hydrogen and chlorine from the industrial process is combined to form hydrogen chloride gas

it's a rather unpleasant gas but it dissolves in water

to produce hydrochloric acid which is a very useful acid it too can be used for cleaning metal but it is also used for

producing chloride salts

these products are very useful and the electrolysis of brine is done on a much larger industrial scale

chlorine is used to kill bacteria and it is soluble in water

if you've ever visited a public swimming pool then you'll be familiar with the smell of chlorinated water and it's also

used to sterilize water in the main water supply

what's more chlorine is one of the main ingredients of bleach which is used in a lot of cleaning products

but this is only scratching the tip of the iceberg as chlorine is used to make dry cleaning ingredients electrical insulators

building materials, refrigerator gasses weed killer pesticides

and is some of the hydrogen and chlorine from the industrial process is combined to form hydrogen chloride gas

it's a rather unpleasant gas but it dissolves in water

to produce hydrochloric acid which is a very useful acid it too can be used for cleaning metal but it is also used for

producing chloride salts

sodium hydroxide is another cleaning product and the most common use for it in the home is for cleaning ovens and unblocking drains

that's a rather amazing collection of uses from our original brine

what's more chlorine is one of the main ingredients of bleach which is used in a lot of cleaning products

but this is only scratching the tip of the iceberg as chlorine is used to make dry cleaning ingredients electrical insulators

building materials, refrigerator gasses weed killer pesticides

and is some of the hydrogen and chlorine from the industrial process is combined to form hydrogen chloride gas

it's a rather unpleasant gas but it dissolves in water

to produce hydrochloric acid which is a very useful acid it too can be used for cleaning metal but it is also used for

producing chloride salts

sodium hydroxide is another cleaning product and the most common use for it in the home is for cleaning ovens and unblocking drains

that's a rather amazing collection of uses from our original brine

what's more chlorine is one of the main ingredients of bleach which is used in a lot of cleaning products

but this is only scratching the tip of the iceberg as chlorine is used to make dry cleaning ingredients electrical insulators

building materials, refrigerator gasses weed killer pesticides

and is some of the hydrogen and chlorine from the industrial process is combined to form hydrogen chloride gas

it's a rather unpleasant gas but it dissolves in water

to produce hydrochloric acid which is a very useful acid it too can be used for cleaning metal but it is also used for

producing chloride salts

sodium hydroxide is another cleaning product and the most common use for it in the home is for cleaning ovens and unblocking drains

that's a rather amazing collection of uses from our original brine

what's more chlorine is one of the main ingredients of bleach which is used in a lot of cleaning products

but this is only scratching the tip of the iceberg as chlorine is used to make dry cleaning ingredients electrical insulators

building materials, refrigerator gasses weed killer pesticides

and is some of the hydrogen and chlorine from the industrial process is combined to form hydrogen chloride gas

it's a rather unpleasant gas but it dissolves in water

to produce hydrochloric acid which is a very useful acid it too can be used for cleaning metal but it is also used for

producing chloride salts

sodium hydroxide is another cleaning product and the most common use for it in the home is for cleaning ovens and unblocking drains

that's a rather amazing collection of uses from our original brine

what's more chlorine is one of the main ingredients of bleach which is used in a lot of cleaning products

but this is only scratching the tip of the iceberg as chlorine is used to make dry cleaning ingredients electrical insulators

building materials, refrigerator gasses weed killer pesticides

and is some of the hydrogen and chlorine from the industrial process is combined to form hydrogen chloride gas

it's a rather unpleasant gas but it dissolves in water

to produce hydrochloric acid which is a very useful acid it too can be used for cleaning metal but it is also used for

producing chloride salts

sodium hydroxide is another cleaning product and the most common use for it in the home is for cleaning ovens and unblocking drains

that's a rather amazing collection of uses from our original brine

what's more chlorine is one of the main ingredients of bleach which is used in a lot of cleaning products

but this is only scratching the tip of the iceberg as chlorine is used to make dry cleaning ingredients electrical insulators

building materials, refrigerator gasses weed killer pesticides

and is some of the hydrogen and chlorine from the industrial process is combined to form hydrogen chloride gas

it's a rather unpleasant gas but it dissolves in water

to produce hydrochloric acid which is a very useful acid it too can be used for cleaning metal but it is also used for

producing chloride salts

sodium hydroxide is another cleaning product and the most common use for it in the home is for cleaning ovens and unblocking drains

that's a rather amazing collection of uses from our original brine

what's more chlorine is one of the main ingredients of bleach which is used in a lot of cleaning products

but this is only scratching the tip of the iceberg as chlorine is used to make dry cleaning ingredients electrical insulators

building materials, refrigerator gasses weed killer pesticides

and is some of the hydrogen and chlorine from the industrial process is combined to form hydrogen chloride gas

it's a rather unpleasant gas but it dissolves in water

to produce hydrochloric acid which is a very useful acid it too can be used for cleaning metal but it is also used for

producing chloride salts

sodium hydroxide is another cleaning product and the most common use for it in the home is for cleaning ovens and unblocking drains

that's a rather amazing collection of uses from our original brine

what's more chlorine is one of the main ingredients of bleach which is used in a lot of cleaning products

but this is only scratching the tip of the iceberg as chlorine is used to make dry cleaning ingredients electrical insulators

building materials, refrigerator gasses weed killer pesticides

and is some of the hydrogen and chlorine from the industrial process is combined to form hydrogen chloride gas

it's a rather unpleasant gas but it dissolves in water

to produce hydrochloric acid which is a very useful acid it too can be used for cleaning metal but it is also used for

producing chloride salts

sodium hydroxide is another cleaning product and the most common use for it in the home is for cleaning ovens and unblocking drains