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Equilibrium Review

Total questions: 43

Worksheet time: 54mins

Name
Class
Date
1.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
2.
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.
3.

Consider the following reaction:

2SO2 + O2 ↔ 2SO3 : ΔΗ = - 197 kJ mol-1

Which of the following will NOT shift the equilibrium position to the right?

a)

Adding more O2

b)

Adding a catalyst

c)

increasing the pressure

d)

Lowering the temperature

4.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
5.

Identify the incorrect statement about achieving equilibrium.

a)

achieved when product and reactant concentrations are equal

b)

achieved when forward and reverse reaction rates are same

c)

achieved when concentration of reactants is stable/constant

d)

achieved when concentration ratio of reactants to products becomes stable, thus fixing the equilibrium constant (equilibrium position)

6.
For the reaction...
N2 (g) +  3 H2 (g) ↔ 2 NH3 (g)

If the pressure in the system is increased,  _______ reaction will be favored.
a)
 the forward
b)
the reverse
c)
neither
7.
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
8.
For the reaction...
heat  +  N2  +  O2  ↔  2NO
If the heat is removed to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
both left and right
d)
neither left nor right
9.

In the given reaction, what happens to [H2O2] if [O2]is decreased?

a)

increase

b)

decrease

c)

stay the same

10.
Which of the two graphs shows a reaction / reactions that reach equilibrium?
a)
The left one.
b)
The right one.
c)
Both of them.
d)
Neither.
11.
2SO2(g)+ O2(g) ⇌ 2SO3(g)
Decreasing volume of container (increasing the pressure)will
a)
shift equilibrium to the right
b)
shift equilibrium to the left
c)
change the value of Kc
d)
have no change on equikliibrium position
12.
N2O4(g) ⇌ 2NO2(g)
What is the concentration equilibrium constant expression?
a)
Kc = [NO2]2 / [N2O4]
b)
Kc = [N2O4] /[ NO2]2
c)
Kc = [N2O4]2 / [NO2]
d)
Kc = [N2O4] x [NO2]2
13.
Le Chatelier's Principle states that if a chemical system at equilibrium is stressed (a change is made)
a)
the system will adjust to increase the stress / imposed change
b)
the system will adjust to reduce the stress / imposed change
c)
the system will not adjust
14.
Given the equation representing a reaction:
N2O4(g) ⇌  2NO2(g)

Which statement describes this reaction at equilibrium?
a)
The concentration of N2O4(g) must equal the concentration of NO2(g).
b)
The concentration of N2O4(g) and the concentration of NO2(g) must be constant  (but not the same as each other)
c)
 The rate of the forward reaction is greater than the rate of the reverse reaction.
d)
The rate of the reverse reaction is greater than the rate of the forward reaction.
15.
T/F: At equilibrium, the amount of reactants and products are the same.
a)
True
b)
False
16.
T/F: At equilibrium, the rate of transfer between the reactants and products is unequal.
a)
True
b)
False
17.
CH4 is added. The reaction will shift:
a)
Right
b)
Left
c)
No Shift
18.
Ne (neon) is added. The reaction will shift:
a)
Right
b)
Left
c)
No Shift
19.
What time is equilibrium reached?
a)
0 s
b)
2000 s
c)
6000 s
20.
Consider the following equilibrium:
2SO2(g) + O2(g) ↔ 2SO3(g) + heat
Which of the following will cause this equilibrium to shift to the left?
a)
Adding a catalyst
b)
Adding some SO2
c)
increasing the volume
d)
increasing the temperature
21.
Which of the following conditions are going to create more NH3?
N2 + 3 H2 ↔ 2 NH3 + 92 kJ
a)
Decreasing Temperature and pressure
b)
Increasing Temperature and Decreasing Pressure
c)
Increasing Temperature and NH3
d)
Decreasing Temperature and N2
22.
Which of the following is not a way to stress a chemical system?
a)
temperature
b)
pressure
c)
time
23.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
24.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
25.
For the reaction...
H2 (g)  + Cl2 (g) <−>  2HCl (g)  +  heat
If the pressure in the system is increased, the equilibrium will _______.
a)
shift left
b)
shift right
c)
not shift
26.

Consider the following reaction. What would be the equilibrium constant expression?

4Br2(g) + CH4(g) ↔ 4HBr(g) + CBr4(g)

a)

[Br2]4 [CH4]/ [HBr]4 [CBr4]

b)

[HBr]4 [CBr4]/ [Br2]4 [CH4]

c)

[HBr ]/ [Br2]4 [CH4]

d)

[HBr]4 [CBr4]/ [Br2]4 [CH4]4

27.
2SO2(g)+O2(g)⇌2SO3(g)
Decreasing volume of container will
a)
shift equilibrium right
b)
shift equilibrium left
c)
change K
d)
have no change
28.
What causes the reaction to go REVERSE
A  + B ↔ C + D + energy
a)
Decreasing D
b)
Increasing C
c)
Decreasing A
d)
Decreasing Temperature
29.
What causes the reaction to go FORWARD
A  + B ↔ C + D + energy
a)
Increasing D
b)
Increasing C
c)
Increasing B
d)
Increasing Temperature
30.

Which change will not shift the position of any reaction at equilibrium?

a)

changing temperature

b)

changing pressure

c)

changing concentration

d)

adding a catalyst

31.

Given the reaction 2NO(g) + 2H2(g) <-> N2(g) + 2H2O(g)


If NO had an initial concentration of .1M and the x value in the ICE chart was found to be .019, what was the equilibrium value of NO?

a)

.138M

b)

.019M

c)

.012M

d)

.062M

32.

Given the reaction 2NO(g) + 2H2(g) <-> N2(g) + 2H2O(g)


At equilibrium, the following concentrations were found:

[NO] = .062, [H2] = .012, [N2] = .019, [H2O] = .138


What is the Keq value?

a)

.0015

b)

650

c)

3.52

d)

.284

33.

Given the reaction: 2NO2(g) <-> N2O4(g)


If the reaction began with nitrogen dioxide and zero concentration of dinitrogen tetraoxide, what would be the Change value for nitrogen dioxide in the ICE chart?

a)

+x

b)

-x

c)

+2x

d)

-2x

34.

Consider the following reaction:

2H2(g) + O2(g) <-> 2H2O(l)

What is the equilibrium constant expression for the reaction?

a)

A

b)

B

c)

C

d)

D

35.

Consider the following reaction:

2Hg(g) + O2(g) <-> 2HgO(s)

The equilibrium constant expression for the reaction is

a)

A

b)

B

c)

C

d)

D

36.

The value of Keq changes when

a)

a catalyst is added.

b)

the temperature changes.

c)

the surface area changes.

d)

the concentration of reactants changes.

37.

Consider the following equilibrium:

H2 (g) + I2(g) <-> 2HI(g) Keq = 50.0

What is the value Keq for the reaction rewritten as:

2HI (g) <-> H2(g) + I2(g) Keq = ?

a)

–50.0

b)

0.0200

c)

25.0

d)

50.0

38.
The idea that when a system at equilibrium is stressed, it will react to relieve that stress and return to equilibrium is known as:
a)
Boyle's Law
b)
Le Chatelier's Principle
c)
Charles Law
d)
Denninger's Law
39.
What states of matter are included when calculating Keq?
a)
Solids and Liquids
b)
Aqueous and Gas
c)
Solids, Liquids, Aqueous solutions and Gases
d)
Aqueous Solutions & Liquids
40.
Which is the correct equilibrium constant expression for the reaction 
CaCO3(s) ⇋ CaO(s) + CO2(g)
a)
[CaO]/[CO2]
b)
[CO2]
c)
1/[CO2]
d)
[CO2][CaO] / [CaCO3
41.
What is the proper Keq for the following reaction? 
   2 NO(g)  +  O2(g) ⇌ 2 NO2(g)
a)
Keq = [NO2]2 / [NO]2[O2]
b)
Keq =  [NO]2[O2] / [NO2]2
c)
Keq = [NO]2[O2][NO2]2
d)
Keq = 2[NO][O2] / 2[NO2]
42.
What is [A] and [B]?
a)
Concentration of Reactants
b)
Concentration of Products
c)
Energy of Reactants
d)
Energy of Products
43.
2SO2(g)+O2(g)⇌2SO3(g)
Removing O2(g) will
a)
shift equilibrium right
b)
shift equilibrium left
c)
decrease temperature
d)
have no change

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