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AP Equilibrium Review

Total questions: 34

Worksheet time: 26mins

Name
Class
Date
1.

An equilibrium constant with a large magnitude indicates…

a)

A very fast reaction

b)

Higher concentration of products at equilibrium

c)

Higher concentration of reactants at equilibrium

d)

Nothing, without considering the stoichiometry of the reaction

2.
Le Chatelier'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
3.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
d)
plasma
4.

For the reaction...

SO2 + O2 ↔ SO3

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

a)

to the reactants

b)

to the products

c)

to reactants and products

d)

to neither reactants nor the products

5.

N2O4(g) ↔ 2 NO2(g)

What is the equilibrium constant expression?

a)

K = [NO2]2/[N2O4]

b)

K = [N2O4]/[NO2]2

c)

K = [N2O4]2/[NO2]

d)

K = [NO2]/[N2O4]2

6.

2 SO2 (g) + O2 (g) ↔ 2 SO3 (g)

Removing O2 (g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

7.
If the equilibrium constant is much greater than one (K >> 1) then
a)
Equilibrium is not established.
b)
Equilibrium lies to the right (products are favored)
c)
Equilibrium lies to the left (reactants are favored)
d)
Neither products or reactants are favored.
8.
If the equilibrium constant is much less than one (K << 1) then
a)
Equilibrium is not established.
b)
Equilibrium lies to the right (products are favored)
c)
Equilibrium lies to the left (reactants are favored)
d)
Neither products or reactants are favored.
9.

What is the equilibrium expression for:

Fe3O4(s) + 4 H2(g) ↔ 3 Fe(s) + 4 H2O(g)

a)

K = ([Fe]3[H2O]4 ) / ([Fe3O4][H2]4)

b)

K = ([Fe3O4][H2]4)/ ([Fe]3[H2O]4)

c)

K = [H2O]4 / [H2]4

d)

K = ([Fe][H2O]) / ([Fe3O4][H2])

10.

For the reaction...

heat + N2 + O2 ↔ 2NO

If NO is removed from the system, the concentration of N2 will _______.

a)

increase

b)

decrease

c)

remain the same

d)

double

11.

For the reaction...

heat + N2 + O2 ↔ 2NO

If the heat is added to the chemical system, the concentration of O2 will _______.

a)

increase

b)

decrease

c)

remain the same

d)

triple

12.

For the reaction...

H2 (g) + Cl2 (g) ↔ 2HCl (g) + heat

If the temperature is cooled, the _________ reaction will be favored.

a)

forward

b)

reverse

c)

forward and reverse

13.
Define chemical equilibrium.
a)
A reaction is reversible.
b)
The concentration of the reactants is equal to the concentration of the products.
c)
The rate of a forward reaction is equal to the rate of the reverse reaction.
d)
The reaction stops and no further change in concentration occurs.
14.
What is the equilibrium-constant expression for 
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
a)
Kc= [CO][H2O] / [CO2][H2]  
b)
Kc= [CO2][H2] / [CO]
c)
Kc= [CO2][H2] / [CO][H2O]
d)
Kc= [CO] / [CO2][H2]  
15.
Equilibrium is a __________ process
a)
Static
b)
Dynamic
c)
Probabilistic
d)
Fictitious
16.
At equilibrium the concentration of all species in the reaction is _________.
a)
Constant
b)
Increasing
c)
Decreasing
d)
Oscillating
17.
Adding a catalyst to a chemical reaction changes the rate of reaction by causing
a)
a decrease in the activation energy
b)
an increase in the activation energy
c)
a decrease in the heat of reaction
d)
an increase in the heat of reaction
18.

When heat is a reactant, the reaction is

a)

exothermic

b)

endothermic

19.

When heat is a product, the reaction is

a)

endothermic

b)

exothermic

20.
A chemical reaction that produces energy is a /an
a)
endothermic reaction
b)
exothermic reaction 
c)
energy
d)
chemical reaction 
21.

Which letter represents the activation energy of the reaction?

a)

A

b)

B

c)

C

d)

D

22.

Which letter represents the overall enthalpy and correctly identifies the reaction type?

a)

C; endothermic

b)

B; endothermic

c)

C; exothermic

d)

B; exothermic

e)

A; endothermic

23.

Which phases should be included in a Kp expression?

a)

only gases

b)

only aqueous

c)

gases and aqueous

d)

everything but solids

24.

Which phases should be included in a KC expression?

a)

only gases

b)

only aqueous

c)

gases and aqueous

d)

everything but solids

25.

Why is it important that reversible reactions are ELEMENTARY?

a)

It's not important

b)

It means the coefficients in the balanced reactions are the orders

c)

It lets us calculate units for K

d)

It lets us calculate Q

26.

nitrate ion

a)

NO3

b)

NO3-1

c)

NO2

d)

NO2-1

27.

How many significant figures are in this number?

200.00

a)

5

b)

4

c)

1

d)

2

28.

What is happening in term of enthalpy?

KBr (s) → KBr (l)

a)

endothermic, +ΔH

b)

exothermic, +ΔH

c)

endothermic, -ΔH

d)

exothermic, -ΔH

29.

Water is boiled. What happens in terms of enthalpy?

a)

endothermic, +ΔH

b)

endothermic, -ΔH

c)

exothermic, +ΔH

d)

exothermic, -ΔH

30.

Given the Kc for a forward reaction, how can you find Kc for the reverse reaction?

a)

Divide Kc by 1

b)

Divide 1 by Kc

c)

Square Kc

d)

Take the square root of Kc

31.
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
32.

2SO2 (g) + O2 (g) ⇌ 2SO3 (g)

Decreasing the volume of container will

a)

shift the system right

b)

shift the system left

c)

change K

d)

have no effect

33.
Which is the reactant - and why?
a)
A, as concentration decreases
b)
B, as concentration decreases
c)
A, as concentration increases
d)
B, as concentration increases
34.
When the system X + 2 Y <=> Z has reached equilibrium, which of the following is TRUE?
a)
Forward reaction and Backward reaction stop.
b)
Forward reaction has sped up and backward reaction has slowed down.
c)
Forward and backward reactions occur at the same rate.
d)
Forward reaction has slowed down and backward reaction has sped up.

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