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Unit 6: Kinetics Review

Total questions: 43

Worksheet time: 46mins

Name
Class
Date
1.
The rate of a chemical reaction is NOT affected by which of the following:
a)
temperature
b)
concentration
c)
particle size (surface area)
d)
All of these affect reaction rates
2.
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.
3.
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
4.

Catalysts permit reactions to proceed along a ___________energy path.

a)

lower

b)

higher

c)

magnetic

d)

psycho's

5.

Smaller particle size allows for a _________ surface area to be exposed for the reaction.

a)

larger

b)

smaller

c)

rectangular

d)

spherical

6.

Increasing the ____ causes the particles (atoms

or molecules) of the reactants to move more quickly so that

they collide with each other more frequently and with more

energy.

a)

Catalyst

b)

Surface Area

c)

Temperature

d)

Concentration

7.

________ is the measure of how much area of an

object is exposed.

a)

Surface Area

b)

Catalyst

c)

Temperature

d)

Concentration

8.

Grains of sugar have a greater _______ than a solid cube of

sugar of the same mass, and therefore will dissolve quicker in water.

a)

Surface Area

b)

Catalyst

c)

Temperature

d)

Concentratrion

9.

Pick the TWO (2) options that will INCREASE the rate of a reaction.

a)

Reducing Heat

b)

Adding Catalyst

c)

Adding Heat

d)

Removing Catalyst

10.

Which of the following will lower the rate

of reaction?

a)

adding an enzyme to the reaction

b)

decreasing the temperature from 40°C to

10°C

c)

breaking a chunk of calcium up into

smaller pieces

d)

increasing the amount of solute

dissolved in a solution

11.
What letter represents the energy of the products?
a)
A
b)
B
c)
C
d)
D
12.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
13.
What letter represents the activation energy?
a)
A
b)
B
c)
C
d)
D
14.
Is this reaction endothermic or exothermic?
a)
endothermic 
b)
exothermic
15.

What is the ΔH of this reaction?

a)

40 kJ

b)

20 kJ

c)

80 kJ

d)

-60 kJ

16.
What is the energy of the activated complex?
a)
75 kJ
b)
225 kJ
c)
300 kJ
d)
225 kJ
17.
What letter represents ΔH?
a)
A
b)
B
c)
C
d)
D
18.
What is the sign of ΔH for all endothermic reactions?
a)
Positive
b)
Negative
19.
What is the activation energy?
a)
40 kJ
b)
20 kJ
c)
100 kJ
d)
60 kJ
20.

What is the change of the heat of the reaction (ΔH)?

a)

-40 kJ

b)

-20 kJ

c)

100 kJ

d)

60 kJ

21.
Which letter represents the activation energy?
a)
B
b)
E
c)
C
d)
D
22.
What is the PE of the reactants?
a)
100 kJ
b)
175 kJ
c)
50 kJ
d)
75 kJ
23.

What is the change of the heat of the reaction (ΔH)?

a)

100 kJ

b)

-175 kJ

c)

-50 kJ

d)

75 kJ

24.

Which system at equilibrium will be least affected by a change in pressure?

a)

3 H2(g) + N2(g) ↔ 2 NH3(g)

b)

2 S(s) + 3 O2(g) ↔ 2 SO3(g)

c)

AgCl(s) ↔ Ag+(aq) + Cl– (aq)

d)

2 HgO(s) ↔ 2 Hg(g) + O2(g)

25.

Given the reaction:  N2(g)+O2(g)+182.6kJ  ↔  2NO(g)N_{2\left(g\right)}+O_{2\left(g\right)}+182.6kJ\ \ ↔\ \ 2NO_{\left(g\right)}  
Which change would cause an immediate increase in the rate of the forward reaction (i.e., cause shift toward products)?

a)

increasing the concentration of NO(g)

b)

increasing the concentration of N2(g)

c)

decreasing the reaction temperature

d)

decreasing the reaction pressure

26.

HEAT + H2CO3 --> CO2 + H2O

If water is decreased, this reaction will shift...

a)

right

b)

left

c)

no change

27.

HEAT + H2CO3 --> CO2 + H2O

If carbonic acid is added, this reaction will shift...

a)

right

b)

left

c)

no change

28.

HEAT + H2CO3 --> CO2 + H2O

If carbon dioxide is added, this reaction will shift...

a)

right

b)

left

c)

no change

29.

HEAT + H2CO3 --> CO2 + H2O

If carbonic acid is removed, this reaction will shift...

a)

right

b)

left

c)

no change

30.
Le Chaltelier's Principle states that if a chemical system at equilibrium is stressed,
a)
the system will adjust to increase the stress
b)
the system will adjust to reduce the stress
c)
the system will not adjust
31.
For the reaction...
SO2(g) + O2(g) <−>  SO3(g)
If the concentration of SO2(g)  is increased, the equilibrium of the reaction will ___________.
a)
shift to the left
b)
shift to the right
c)
not shift
32.
For the reaction...
SO2(g) + O2(g) <−>  SO3(g)
If the equilibrium shifts to the right, the concentration of O2(g) will ___________.
a)
increase
b)
decrease
c)
remain the same
33.

What is collision theory?

a)

Molecules must collide in the correct orientation with enough energy to bond.

b)

Molecules need enough energy to collide and react.

c)

Atoms constantly collide and react.

d)

The minimum energy needed for atoms to react

34.

Which PE Diagram represents an endothermic reaction?

a)

A

b)

B

35.

Which PE Diagram represents an exothermic reaction?

a)

A

b)

B

36.

What is the purpose of a catalyst?

a)

Helps to slow down a reaction

b)

Raises the activation energy

c)

Lowers the activation energy

d)

Is consumed by the reaction

37.

What factors effect rate of reaction?

a)

Temperature, Concentration, Pressure and Energy

b)

Surface Area, Concentration, Energy and Pressure

c)

Temperature, Pressure, Concentration and Surface area

d)

Pressure, Surface area, Density and Energy

38.

What criteria must be met for reactant collisions to result in a successful product?

a)

The reactants must collide with each other

b)

The reactants must collide with enough energy and be in the right positions

c)

The reactants must have enough energy to form the activated complex

39.
More collisions correspond to a: 
a)
Faster reaction rate  
b)
Slower reaction rate
c)
Constant reaction rate 
d)
None of the above
40.
Which of the following is/are the fundamental idea(s) of collision theory?
a)
Molecules react by colliding together
b)
The effective collisions must occur with certain minimum amounts of energy 
c)
In a large sample, the greater the number of effective collisions, and the faster the rate of reaction
d)
All of the above
41.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
42.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Neutralise the reaction
d)
increase collision between the particles thus increasing the rate.
43.
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

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