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Chem Unit 10 Review: Reaction Rates and Equilibrium

Total questions: 20

Worksheet time: 17mins

Name
Class
Date
1.

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

2.

Which factors increase the rate of a reaction?

a)

increasing temperature

b)

increasing concentration

c)

increasing total surface area

d)

All of these

3.
Identify the labels (a) and (b) on the graph.
a)
a is concentration of reactants and b is the concentration of product
b)
a is concentration of product and b is the concentration of reactant
c)
a is the volume of reactants and b is the volume of product
d)
a the mass of reactants and b is the mass of product
4.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
5.

Which of the reaction pathway shows the catalysed reaction?

a)

1

b)

2

6.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by making them more available

c)

by giving them more energy

7.

What is the name given to a catalyst in the human body?

a)

Biology

b)

Catalyst

c)

Chemical

d)

Enzyme

8.

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

9.

How could we make this reaction happen more quickly?

a)

Decrease the concentration of the acid

b)

crush the chalk to increase the surface area

c)

Put the test tube in an ice bath

10.
The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Which pathway is slower and why?
a)
Red, because the activation energy is larger
b)
Blue, because the activation energy is lower
c)
both reaction progress at the same rate
11.
What letter represents the activation energy?
a)
A
b)
B
c)
C
d)
D
12.
Under the collision theory, the particles must collide with  ____ and ____ for a reaction to occur.
a)
sufficient rate and sufficient energy
b)
sufficient surface area and correct orientation
c)
sufficient catalyst and sufficient energy
d)
sufficent energy and correct orientation
13.

Is the following reaction endothermic or exothermic

a)

endothermic

b)

exothermic

14.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
15.

The rate of a chemical reaction normally

a)

increases as temperature decreases.

b)

decreases when a catalyst is added.

c)

increases as reactant concentration increases.

d)

decreases as reactant concentration increases.

16.

Which of the following statements is CORRECT for a reaction at an equilibrium?

a)

The rate of forward and reverse reactions are equal.

b)

The concentrations of product and reactant are equal.

c)

The forward and reverse reactions will stop.

d)

Always occur in an open system.

17.
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
18.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Adding SO2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase rate of reaction

d)

have no change

19.

2SO2(g) + O2(g) ⇌ 2SO3(g) + Heat


Removing O2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

20.

2SO2(g) + O2(g) ⇌ 2SO3(g) + Heat


Using a catalyst

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase the rate of reaction

d)

have no change

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