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Y11 iG Chem U20-21 Rates and Equil

Total questions: 101

Worksheet time: 7hrs 38mins

Name
Class
Date
1.

Label these two energy diagrams correctly. Be aware you will have to DRAW these from memory on your GCSE Test

a)Activation Energy (endo)
b)Activate Exo
c)Transition State (Activated State)
d)Positive AH (Enthalpy)
e)Negative AH (Enthalpy)
f)Reactants
g)Products
h)Exothermic Diagram
i)Endothermic Diagram
1
2
3
4
5
6
7
8
9
1)
2)
3)
4)
5)
6)
7)
8)
9)
2.
a)

1 and 3

b)

1 and 4

c)

2 and 3

d)

2 and 4

3.
a)

A

b)

B

c)

C

d)

D

4.

Why does a higher temperature increase the rate of a reaction?

a)

it increases both the frequency and energy of particle collisions

b)

it only increases the frequency of particle collisions

c)

it only increases the energy of particle collisions

d)

it reduces the activation energy of the reaction

5.

Grinding a effervescent tablet into powder increases the rate of reaction due to increased

a)

concentration

b)

surface area

c)

temperature

d)

reactants

6.

Adding a catalyst ___________ the activation energy.

a)

Raises

b)

Lowers

c)

Doesn't affect

d)

Inreases

7.

The minimum amount of energy needed for colliding particles to react is called

a)

Chemical Energy

b)

Kinetic Energy

c)

Activation Energy

d)

Potential Energy

8.
The graph shows how the total volume of a gas given off from a reaction changes with time. In which time interval is least gas given off? 
a)
A
b)
B
c)
C
d)
D
9.
Why does a catalyst increase the rate of reaction?
a)
it produces extra energy for the reactants
b)
it increases the speed of the reactant particles
c)
it increases the frequency of particle collisions
d)
it reduces the activation energy of the reaction 
10.
Why don't all collisions between particles cause a reaction?
a)
the particles also need to collide with a catalyst
b)
not all the particles collide with enough energy
c)
not all the particles collide at a high enough temperature
d)
the particles need to collide with each other twice
11.
What makes an effective collision?
a)
When molecules collide.
b)
When molecules collide with the proper orientation.
c)
When molecules collide with proper orientation and enough kinetic energy.
d)
High Temperature.
12.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

13.

Why does a higher temperature increase the rate of a reaction?

a)

it increases both the frequency and energy of particle collisions

b)

it only increases the frequency of particle collisions

c)

it only increases the energy of particle collisions

d)

it reduces the activation energy of the reaction

14.

How is this equipment being used to measure the rate of reaction?

a)

The gas syringe measures how much gas is produced in a certain time

b)

The reaction mixture will increase in volume in a certain time

15.

The rates of some chemical reactions can be measured by using the apparatus shown. For which reaction is this apparatus suitable?

a)

MgCO3 + 2HCl -> MgCl2 + CO2 + H2O

b)

Mg + ZnCl2 -> MgCl2 + Zn

c)

MgCl2 + 2NaOH -> Mg(OH)2 + 2NaCl

d)

MgO + 2HCl -> MgCl2 + H2O

16.

When you react sodium thiosulfate and hydrochloric acid, the solution turns cloudy. This is because...

a)

a sodium precipitate is produced

b)

a sulfur precipitate is produced

17.

Which solution show a higher concentration (left or right)?

a)

left

b)

right

c)

both the same

18.

The more concentrated the sodium thiosulfate solution, the less time is taken for the cross to become no longer visible. Give two reasons why.

a)

Particles are more spread out

b)

Particles collide more frequently

c)

Particles have more energy

d)

Particles move more quickly

e)

There are more particles in a fixed volume

19.
What is the rate of reaction?
a)
How fast a reaction is 
b)
How big a reaction is
c)
How loud a reaction is
d)
How much gas a reaction produces
20.

Which factors affect the rate of a reaction?

a)

temperature

b)

concentration

c)

surface area

d)

pressure

e)

add a catalyst

21.

Which of the following explains the meaning of effective collision?

a)

The collision where its energy is less than the activation energy

b)

The collision that has a low energy

c)

The collision which takes place before a reaction

d)

The collision that causes a reaction

22.

Increase in temperature causes the particles to

a)

slow down

b)

move faster

c)

stay apart from each other

d)

move in the correct order

23.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
24.

Why does using an acid with a

higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of reactant particles

d)

it increases the frequency of collision

25.

A temperature increase causes the particles ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

26.

Why does a higher temperature increase the rate of a reaction?

a)

It increases both the frequency collision and energy of reactant particles

b)

It only increases the frequency of collision

c)

It only increases the energy of reactant particles

d)

It reduces the activation energy of the reaction

27.

Grinding an effervescent tablet into powder increases the rate of reaction due to increase of

a)

concentration

b)

total surface area

c)

temperature

d)

size

28.

Which factors increase the rate of a reaction?

a)

increasing temperature

b)

increasing concentration of solutions like acids

c)

increasing total surface area of solids

d)

All of these

29.

Increasing pressure causes the reacting particles

a)

to bond together

b)

to repel from each other

c)

gain more kinetic energy

d)

to move closer together

30.

Increasing the temperature gives particles more __________.

a)

time

b)

energy

c)

space

d)

frequency

31.

You add more bodies into a "mosh pit" to hope for more collisions. You have increased

a)

temperature

b)

concentration

c)

pressure

d)

catalyst

32.

You make a space much smaller by increasing the ________________ hoping to increase the reaction rates.

a)

temperature

b)

concentration

c)

catalyst

d)

pressure

33.

Why does breaking up a solid reactant increase the rate of reaction?

a)

it creates more solid

b)

it creates more energy

c)

it increases the total surface area

d)

it increases the concentration

34.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of collisions

35.

The following equation shows the reaction between calcium carbonate, CaCO3 and hydrochloric acid, HCl:


CaCO3(aq) + 2HCl(aq) → CaCl2(aq) + CO2 (g)­­ + H2O(l)


Which of the following is the suitable method to determine the rate of reaction?

a)

Change in the temperature of the solution with time

b)

Change in the volume of carbon dioxide gas with time

c)

Change in the mass of water with time

d)

Change in the concentration of hydrochloric acid with time

36.

Diagram 4 shows the graph of volume of carbon dioxide gas against time when 5 g of marble chips is added to

50 cm3 of 0.2 mol dm-3 hydrochloric acid.


At what time the rate of reaction the highest?

a)

t1

b)

t2

c)

t3

d)

t4

37.

Diagram 7 shows a graph of the volume of gas produced against time for the reaction between zinc granules and hydrochloric acid.


The gradient of the graph decreases with time because

a)

catalyst is not used

b)

volume of mixture decreases

c)

temperature of reaction decreases

d)

concentration of hydrochloric acid decreases

38.

The equation represents the reaction between sodium carbonate and hydrochloric acid.

Na2CO3 + 2 HCl → 2 NaCl + H2O + CO2


The mass of the beaker and its contents is plotted against time.

Which graph represents what happens when sodium carbonate reacts with an excess of dilute hydrochloric acid?

a)
b)
c)
d)
39.

Which of the following is the meaning of activation energy?

a)

The maximum energy that the particles need to produce effective collision

b)

The amount of energy used by the particles during a collision

c)

The minimum amount of energy that particles must have in order to react

d)

The amount of kinetic energy of molecules during a collision

40.
Identify the concentrations of hydrochloric acid used in the experiment.
a)0.5 mol/dm³
b)1.0 mol/dm³
c)2.0 mol/dm³
1
2
3
1)
2)
3)
41.
Identify the sizes of magnesium pieces mentioned in the text.
a)large
b)small
c)very small
d)Time increases, same amount produced
e)Time decreases, more amount produced
f)Time increaeses, less amount produced
g)Time stays the same, same amount produce
1
2
3
4
1)
2)
3)
4)
42.

Label the first column for A,B,C

a)A- increases
b)A- decreases
c)A- no change
d)B- decreases
e)B- increases
f)B- no change
g)C- increases
h)C- decreases
i)C- no change
1
2
3
1)
2)
3)
43.

Label the first column for A,B,C

a)D- increases
b)D- decreases
c)D- no change
d)forward rxn is endothermic
e)forward reaction is exothermic
1
2
1)
2)
44.

Explain,what happens to the rate of a reaction when the temperature is reduced.

1. ​ ​ The rate or speed... (a)  

  1. ​ 2. In terms of collisions..​ (b)  

  2. 3. In terms of energy... ​ (c)   o

Choose from the below words
decreases and particles have less energy
fewer collisions occur per second / per unit time
fewer particles have enough energy to react
increases and particles have less energy
more collisions occur per second /per unit time
more particles have enough energy to react
45.

Correctly define a catalyst.

a)increases rxn rate
b)decreases rxn rate
c)doesn't change rxn rate
d)provides alt lower energy pathway
e)provides lower original energy pathway
f)remains unchanged at end of rxn
g)changes by the end of the reaction
h)is a transition metal
i)shifts the equilibrium to forward rxn
j)shifts the equilibrium to the backwards
1
2
3
1)
2)
3)
46.

Corrctle predict equilibrium

a)A - increases
b)B - decreases
c)C -decreases
d)D - decreases
e)A - decreases
f)B - increases
g)C -increases
h)D - increases
i)no change
1
2
3
4
1)
2)
3)
4)
47.

Describe how the graph shows the rate of this rxn decreases as time increases.

a)gradient of the line decreases
b)product stops being produced
c)B1 - concentration of particles decrease
d)B1 - concentration of particles increase
e)B2-lower frequency of collisions
f)B2-higher frequency of collisions
g)B2-less collisions
h)orange line
i)pink line
j)blue line
1
2
3
4
1)
2)
3)
4)
48.

Correctly answer the questions

a)oxygen gas is escaping
b)hydrogen peroxide is escaping
c)rate decreases and then stops
d)rate increases and then stops
e)rate decreases and continues
f)prevent reactant from escaping
g)prevent gas from escaping
h)to allow gas to escape
1
2
3
1)
2)
3)
49.

Describe two features of an equilibrium

a)A1-constant concentration
b)A2-equal rates forward and back
c)A1-equal concentration
d)A2-constant rate forward and backwards
e)A2-diff rate forward and backwards
f)A1-Diff concentration
1
2
1)
2)
50.

Explain what happens to equilibrium when temp and pressure are changed.

a)T1-Shifts to reactants
b)T1-Shifts to products
c)T2-reverse rxn is endo
d)T2-forward rxn is exo
e)P1-Shifts to products
f)P1-Shifts to reactants
g)P2-fewer moles on product side
h)P2-fewer moles on reactant side
i)P2-more moles on product side
1
2
3
4
1)
2)
3)
4)
51.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
52.
When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in
a)
Chemical Equilibrium
b)
Chemical Balance
c)
Chemical Constant
d)
Chemical Reaction
53.

A chemical reaction where the reactants form products that, in turn, react together to give the reactants back.

a)

reversible reaction

b)

irreversible reaction

c)

decomposition reaction

d)

synthesis

54.
For the reaction...
SO2 + O2  <=>  SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
a)
to the left
b)
to the right
c)
to the left and right 
d)
neither left nor right
55.
For the reaction...
SO2 + O2 <=>  SO3
If the equilibrium position shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
56.
For the reaction...
N2  +  O2  <=>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
57.

For the reaction...

N2 (g) + 3 H2(g) <=> 2 NH3 (g)


If the volume is decreased, which substance(s) will increase in concentration?

a)

N2 (as 2 mol gas → 4 mol gas)

b)

H2 (as 2 mol gas → 4 mol gas)

c)

N2 and H2 (as 2 mol gas → 4 mol gas)

d)

NH3 (as 4 mol gas → 2 mol gas)

58.

For the reaction...

N2 + O2 <=> 2NO + 182kJ (the 182 kJ means heat)

If the temperature is increased the equilibrium position will shift _______.

a)

to the left

b)

to the right

c)

to the left and right

d)

neither left nor right

59.
Le Chatelier's Principle states that.... 
If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium................
a)
moves to increase the change
b)
moves to counteract the change
c)
does not change
60.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
61.
For the reaction...
H2 (g)  + Cl2 (g) <=>  2HCl (g)  +  heat
If the pressure in the system is increased, the equilibrium position will _______.
a)
shift to the left
b)
shift to the right
c)
not shift position at all as 2 mol gas <=> 2 mol gas
62.

For the reaction...

N2 (g) + 3 H2(g) ⇌ 2 NH3 (g)


If the pressure in the system is increased, which substance(s) will increase in concentration?

a)

N2

b)

H2

c)

N2 and H2

d)

NH3

63.

What is the effect of increasing the pressure on the following equilibrium: 2NO(g) + O2 (g) ⇌2NO2(g)?

a)

The yield of NO2 increases

b)

The yield of NO2 decreases

c)

The reaction is slower

d)

The concentration of O2 increases.

64.

2SO2(g) + O2(g) ⇌ 2SO3(g)

Removing O2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

65.

2SO2(g) + O2(g) ⇌ 2SO3(g)

Adding SO3(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase K

d)

have no change

66.

H2(g) + Cl2(g) ⇌ 2HCl(g) + heat

What will happen to the equilibrium if the temperature is increased?

a)

equilibrium shifts right

b)

equilibrium shifts left

c)

You cannot predict the effect

d)

no change

67.

What is Le Chatelier's principle?

a)

A principle that explains the behavior of gases at high pressures

b)

A cooking technique used to prepare French cuisine

c)

A mathematical formula for calculating equilibrium constants

d)

Principle that describes how a system at equilibrium responds to changes in its conditions

68.

3H2 (g) + N2 (g) ⇌ 2NH3 + heat

When a system at equilibrium is subjected to a change, how does it respond according to Le Chatelier's principle?

a)

It shifts the equilibrium position to counteract the change.

b)

It reverses the change

c)

It accelerates the change

d)

It remains unchanged

69.

3H2 (g) + N2 (g) ⇌ 2NH3 + heat

If the concentration of a reactant is increased, according to Le Chatelier's principle, what will happen to the equilibrium position?

a)

The equilibrium position will remain unchanged.

b)

The equilibrium position will shift to the left.

c)

The equilibrium position will disappear.

d)

The equilibrium position will shift to the right.

70.

3H2 (g) + N2 (g) ⇌ 2NH3 + heat

If the temperature of a system at equilibrium is decreased, what will be the effect on the equilibrium position?

a)

The equilibrium position will reverse

b)

The equilibrium position will remain the same

c)

The equilibrium position will shift to the right

d)

The equilibrium position will shift to the left

71.

What is the effect of adding a catalyst to a system at equilibrium, according to Le Chatelier's principle?

a)

It shifts the equilibrium to the left

b)

It slows down the attainment of equilibrium

c)

It has no effect on the equilibrium position

d)

It speeds up the attainment of equilibrium without affecting the equilibrium position.

72.

In a reversible reaction, if the pressure is increased, what will be the effect on the equilibrium position?

a)

The equilibrium position will not be affected by the pressure change.

b)

The equilibrium position will shift towards the side with more solid reactants.

c)

The equilibrium position will shift towards the side with fewer moles of gas.

d)

The equilibrium position will shift towards the side with more moles of gas.

73.

What is the effect of increasing the temperature on a system at equilibrium, according to Le Chatelier's principle?

a)

The equilibrium position will shift to the direction of the endothermic rxn

b)

The equilibrium position will remain unchanged

c)

The equilibrium position will disappear

d)

The equilibrium position will shift to the direction of the exothermic rxn

74.

What happens to the equilibrium position in a reversible reaction when the concentration of products is increased?

a)

The equilibrium position will shift to the left

b)

The equilibrium position will remain unchanged

c)

The equilibrium position will disappear

d)

The equilibrium position will shift to the right

75.

How does the addition of a catalyst affect the equilibrium position in a chemical reaction, according to Le Chatelier's principle?

a)

It shifts the equilibrium to the left

b)

It slows down the attainment of equilibrium

c)

It has no effect on the equilibrium position

d)

It speeds up the attainment of equilibrium without affecting the equilibrium position.

76.

What is dynamic equilibrium?

a)

The reaction goes forward

b)

The reaction goes backward

c)

The rate of forward and backward reaction is equal

d)

The equilibrium is dynamite

77.

Which of the following does not affect the position of equilibrium?

a)

Temperature

b)

Pressure

c)

Particle Size

d)

Concentration

78.

How does a catalyst affect the position of the equilibrium?

a)

It does not. It only increases the rate of reaction.

b)

Position of equilibrium will shift to the right.

c)

Position of equilibrium will shift to the left.

d)

The reaction would be slower.

79.

3H2 (g) + N2 (g) ⇌ 2NH3 + heat

What would be the effect of increasing the temperature to the equilibrium of an exothermic reaction?

a)

equilibrium shifts to the left

b)

equilibrium shifts to the right

c)

no change in position of equilibrium

80.

2NH3 + heat ⇌ 3H2 (g) + N2 (g)

What would be the effect of increasing the temperature to the equilibrium of an endothermic reaction?

a)

equilibrium shifts to the left

b)

equilibrium shifts to the right

c)

no change in position of equilibrium

81.

3H2 (g) + N2 (g) ⇌ 2NH3 + heat

What would be the effect of increasing the concentration of the product on the position of the equilibrium?

a)

equilibrium shifts to the left

b)

equilibrium shifts to the right

c)

no change in position of equilibrium

82.

3H2 (g) + N2 (g) ⇌ 2NH3 + heat

What would be the effect of decreasing the concentration of the reactant on the position of the equilibrium?

a)

equilibrium shifts to the left

b)

equilibrium shifts to the right

c)

no change in position of equilibrium

83.

3H2 (g) + N2 (g) ⇌ 2NH3 + heat

When pressure is increased, the position of the equilibrium will shift to the side that has...

a)

less number of gaseous molecules

b)

more number of gaseous molecules

84.

3H2 (g) + N2 (g) ⇌ 2NH3 (g) ΔH = −197 kJ/mol

Which of the following factors would shift the equilibrium position to the right? (Choose 2)

a)

increase concentration of nitrogen gas

b)

increase temperature of the equilibrium

c)

increase pressure of the equilibrium

d)

Presence of a catalyst

85.

H2 (g) + I2 (g) ⇌ 2HI (g)

What would be the effect of increasing the pressure on the position of equilibrium?

a)

equilibrium shifts to the right

b)

equilibrium shifts to the left

c)

no change in position of equilibrium

86.

Provide an example of a reversible reaction.

a)

Formation of water from hydrogen and oxygen gas

b)

Combustion of methane

c)

Decomposition of water into hydrogen and oxygen gas

d)

Photosynthesis

87.

Heat + 1 N2O4 → 2 NO2


What will happen when the temperature is increased?

a)

Position of equilibrium will shift to left and become lighter in color

b)

Position of equilibrium will shift to right and become more brown

c)

No change in position of equilibrium

d)

Position of equilibrium will shift to right and become lighter in color

88.
At what time (in seconds) is equilibrium established?
a)
0 seconds
b)
1 second
c)
5 seconds
d)
10 seconds
89.
At what time does the reaction reach equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
90.

Answer part b.

a)T1-equilibrium shifts to reactants
b)T1-equilibrium shifts to products
c)T2-reaction is exothermic
d)T2-reaction is endothermic
e)P1-equilibrium shifts to products
f)P2-more particles on reactant side
g)P1-equilibrium shifts to reactants
h)P2-more particles on product side
1
2
3
4
1)
2)
3)
4)
91.

Correctly predict the position of equilibrium.

a)T1-equilibrium shifts to products
b)T1-equilibrium shifts to reactants
c)T2-reaction is exothermic
d)T2-reaction is endothermic
e)P1-equilibrium shifts to reactant
f)P2-more particles on reactant side
g)P1-equilibrium shifts to products
h)P2-more particles on product side
1
2
3
4
1)
2)
3)
4)
92.

Correctly predict the position of equilibrium. (Make sure you are able to explain it too!)

a)T1-increases
b)T1-decreases
c)T2-decreases
d)T2-increases
e)P1-decreases
f)P1-increases
g)P2-decreases
h)P2-increases
1
2
3
4
1)
2)
3)
4)
93.

Explain why this reaction is not carried out at these temperatures.

a)rxn would be too slow
b)rxn would be too fast and explode
c)yield of ethanoic acid would be too low
d)yield of ethanoic acid would be too high
e)the enzymes would start to break down
1
2
1)
2)
94.

Correctly predict the shift in equilibrium.

a)C1-increases
b)C1-decreases
c)no change
d)C2-increases
e)C2-decreases
f)P1-decreases
g)P1-increases
h)P2-decreases
i)P2-increases
1
2
3
4
1)
2)
3)
4)
95.

Explain what would most likely be a suitable catalyst.

a)cobalt
b)aluminium
c)calcium
d)magnesium
e)potassium
f)transition metal multiple stable states
g)alkali metal most reactive to be stable
h)smallest metal with 2 outer e-
i)not too reactive and has two electrons
j)has the highest charge of +3
1
2
1)
2)
96.

Correctly answer the following questions with this reaction we've studied.

a)white
b)blue
c)green
d)black
e)heating
f)cooling
g)adding water
h)5H2O
i)H2O
j)10OH
1
2
3
4
1)
2)
3)
4)
97.

Correctly predict and explain the shift (if any) on the equilibrium given the change in conditions.

a)A1-equil shifts to products
b)A1-equil shifts to reactants
c)A2-fewer moles on product side
d)B1-equil shifts to reactants
e)B1-equil shifts to products
f)B2-fwd rxn is exo
g)B2-fwd rxn is endo
h)A2-fewer moles on reactant side
i)no change
1
2
3
4
1)
2)
3)
4)
98.

Correctly EXPLAIN the following:

a)NO2 particles are forced closer together
b)lower number of moles on reactant side
c)lower number of moles on product side
d)NO2 particles are forced further away
e)N2O4 particles are forced closer 
1
2
1)
2)
99.

Correctly predict what happens to this rxn when temperature changes.

a)shifts to the product side
b)shifts to the reactant side
c)no change
d)rate of fwd rxn increases
e)rate of fwd rxn decreases
f)rate of bwd rxn decreases
1
2
3
1)
2)
3)
100.

Correctly explain what you would see and why.

a)A1-color is paler
b)A1-color is darker
c)A2-equil shifts right
d)A2-equil shifts left
e)A3-fewer moles on right
f)A3-fewer moles on left
g)B1-more N2O4 forms
h)B1-more NO2 forms
i)B2-fwd rxn is exo
j)B2- bwd rxn is exo
1
2
3
4
5
1)
2)
3)
4)
5)
101.

Correctly show you have studied this reaction.

a)NH4Cl (s)
b)reforming NH4Cl(s)
c)ammonia and HCl gas
d)reforming NH3 and HCl
e)endothermic (absorbsheat)
f)exothermic (releases heat)
g)Cooler area, chemicals are releasingheat
h)hotter part, chemicals are absorbingheat
1
2
3
4
5
6
7
1)
2)
3)
4)
5)
6)
7)

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