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ICP Unit 5 Review

Total questions: 50

Worksheet time: 1hrs 4mins

Name
Class
Date
1.

Which observation would most likely indicate that an endothermic reaction has occurred?

a)

A color change

b)

The production of gas bubbles

c)

An increase in temperature of the surroundings

d)

A decrease in temperature of the surroundings

2.

Before a chemical reaction, the total mass of two reactants is measured to be 65 grams. After the reaction, what should be the total mass of the products?

a)

0 grams

b)

25 grams

c)

45 grams

d)

65 grams

3.

The idea that matter is neither created nor destroyed in chemical reactions is known as the:

a)

Law of conservation of chemicals.

b)

Law of conservation of energy.

c)

Law of conservation of mass.

d)

Second law of thermodynamics.

4.

Copper chloride (CuCl2) and aluminum react to produce aluminum chloride (AlCl3) and copper. Which of the following is the correctly balanced chemical equation for this reaction?

a)

CuCl2 + Al → AlCl3 + Cu

b)

3CuCl2 + Al→ AlCl3 + 2Cu

c)

3CuCl2 + 2Al → 2AlCl3 + 3Cu

d)

CuCl2 + 3Al → AlCl3 + 2Cu

5.

Give the reactants in the following equation:

CH4 + 2O2 → CO2 + H2O

a)

CH4 and CO2

b)

2O2 and CO2

c)

CH4 and 2O2

d)

2O2 and H2O

6.

Give the products in the following equation:

CH4 + 2O2 → CO2 + H2O

a)

CH4 and CO2

b)

2O2 and CO2

c)

2O2 and H2O

d)

CO2 and H2O

7.

Is this equation balanced?

N2 + 3H2 → 2NH3

a)

Yes - it is balanced

b)

No - it is not balanced

8.

Is this equation balanced?

Mg + O2 → MgO

a)

Yes - it is balanced

b)

No - it is not balanced

9.
2 NaBr + 1 Ca(OH)2 ----> 1 CaBr2 + 2 NaOH
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
10.
2 NH3+ 1 H2SO4 ----> 1 (NH4)2SO4
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
11.
3 Pb + 2 H3PO4 ----> 3 H2 + 1 Pb3(PO4)2
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
12.
1 Li3N + 3 NH4NO3 ----> 3 LiNO3 + 1 (NH4)3N
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
13.
CaCO3 ----> CaO + CO2
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
14.
__Al + __Fe3N2 -->__AlN + __Fe
a)
already balanced
b)
4,2,4,6
c)
2,1,2,3
d)
1,2,1,3
15.
__Na + __Cl2 --> __NaCl
a)
1,1,2
b)
2,1,2
c)
2,1,1
d)
already balanced
16.
__NaClO3 --> __NaCl + __O2
a)
2,2,2
b)
2,2,3
c)
3,2,2
d)
1,2,3
17.

What happens in an Endothermic reaction?

a)

More energy is released

b)

Energy is used up

c)

The substance heats up

d)

The temperature of the substance stays the same

18.
What happens in an Exothermic reaction?
a)
More energy is released
b)
Less energy is released
c)
The substance's temperature stays the same
d)
The substance gets colder
19.

What type of reactions is this:

C3H8 + O2 --> H2O + CO2

a)

Synthesis (combination)

b)

Decomposition

c)

Single replacement

d)

Combustion

20.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
d)
plasma
21.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
22.
What are the two factors to look for when determining if the reaction is at equilibrium?
a)
Forward reaction rate is faster than the reverse and concentrations are equal
b)
Forward and reverse reaction rates are equal and concentration is constant
c)
Forward and revers reaction rates are equal and concentration is equal
d)
Forward reaction rate is faster than the reverse and concentration is equal
23.
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)
Stoichiometry
d)
Chemical Reaction
24.

For the reaction...

SO2 + O2 ⇌ SO3

If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.

a)

left

b)

right

c)

left and right

d)

neither left nor right

25.

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

26.
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
27.

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

28.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
29.
The rate of a reaction increases as temperature__________________.
a)
Decreases
b)
Increases
c)
Stays the Same
30.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
31.
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
32.
Smaller particle size allows for a _________ surface area to be exposed for the reaction.
a)
larger
b)
smaller
33.
The ___________ the surface area of the reactants, the faster the reaction rate.
a)
larger 
b)
smaller
34.
Increasing the temperature will increase the kinetic energy of particles, therefore increasing the collisions between particles.
a)
false
b)
true
35.

Why are chemical equations always balanced? Select ALL that apply.

a)

Matter cannot be created.

b)

Matter cannot be destroyed.

c)

Matter can only be rearranged/conserved.

d)

Matter doesn't matter.

36.
3 HBr + 1 Al(OH)3 ----> 3 H­2O + 1 AlBr3
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
37.
Na3PO4 + 3 KOH ----> 3 NaOH + K3PO4
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
38.
Pb + FeSO4 ----> PbSO4 + Fe
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
39.
MgCl2 + Li2CO3 ----> MgCO3 + 2 LiCl
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
40.
P4 +  3 O2 ----> 2 P2O3
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
41.
2 AgNO3 + Cu ----> Cu(NO3)2 + 2 Ag
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
42.
2 C5H5 + Fe ----> Fe(C5H5)2
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
43.
SeCl6 + O2 ----> SeO2 + 3Cl2
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
44.
2 MgI2 + Mn(SO3)2 ----> 2 MgSO3 + MnI4
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
45.
O3  ----> O. + O2
a)
Synthesis (or combination)
b)
Decomposition
c)
Single displacement
d)
Double displacement
46.
CxHy +O2 --> H2O + CO2
a)
Decomposition
b)
Double replacement
c)
Combustion
d)
Single Replacement
47.
One reactant into several products.
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
48.
One element replaces another in a compound.
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
49.
This pictures simulates what type of reaction?
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
50.

Combustion reactions will always involve

a)

Oxygen and a solid

b)

Liquid nitrogen and heat

c)

Oxygen and heat/energy

d)

CO and H2O

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