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Chemical Equilibrium and Le Chatelier's

Total questions: 60

Worksheet time: 5hrs 0mins

Name
Class
Date
1.
The following factors affect the position of equilibrium EXCEPT
a)
Concentration
b)
Pressure
c)
Temperature
d)
States of matter
2.

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

3.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Increasing the temperature will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

4.

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

5.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Adding SO3(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase K

d)

have no change

6.

2SO2(g)+1O2(g) ⇌ 2SO3(g) + Heat


Increasing the volume of the container will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

slow rate of reaction

d)

have no change

7.

2SO2(g)+1O2(g) ⇌ 2SO3(g) + Heat


Increasing the pressure on the system will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

slow rate of reaction

d)

have no change

8.

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

9.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
10.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
d)
plasma
11.
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
12.
For the reaction...
SO2 + O2 <−>  SO3
If the equilibrium shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
13.

N2 (g) + 3H2 (g) < -> 2NH3 (g) + Heat

Removing H2

a)

Shift Left

b)

Shift Right

14.

N2 (g) + 3H2 (g) < -> 2NH3 (g) + Heat

add N2

a)

Shift Left

b)

Shift Right

15.

Given the reaction at equilibrium:

2SO2(g) +O2(g) <--> 2SO3(g) + HEAT

Which change will shift the equilibrium to the right?

a)

decrease the pressure

b)

increasing the pressure

c)

decreasing the amount of SO2(g)

d)

decreasing the amount of O2(g)

16.

2SO2(g)+1O2(g) ⇌ 2SO3(g) + Heat


Increasing the volume of the container will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

slow rate of reaction

d)

have no change

17.

When writing an endothermic reaction, heat energy is stated as a

a)

product

b)

reactant

18.

How do catalysts increase the rate of reaction?

a)

The frequency of collisions is increased

b)

The activation energy is lowered

c)

The energy of collisions is increased

d)

Both the frequency and energy of collisions is increased

19.
What is the activation energy?
a)
The quantity of heat absorbed in a reaction
b)
The minimum energy needed to begin a reaction
c)
The energy given off after reactants collide.
d)
The energy difference between reactants and products
20.

For the reaction...

heat + N2 + O2 ↔ 2NO

If the heat is added to the chemical system, the equilibrium will shift _______.

a)

forward

b)

reverse

c)

no shift

21.

A chemical reaction that releases energy is an

a)

endothermic reaction

b)

exothermic reaction

c)

energy

22.

At what time (in seconds) is equilibrium established?

a)

0 seconds

b)

1 second

c)

5 seconds

d)

10 seconds

23.

At room temperature, the reaction of H2 with Cl2 to make HCl has an equilibrium constant of 2.4×1033.

If 0.010 mol H2 is in a container with 0.010 mol Cl2 and 1.0 mol HCl, which way will the reaction shift to achieve equilibrium? HINT: CALCULATE Q!

a)

To the products (right)

b)

To the reactants (left)

c)

Neither; the reaction is at equilibrium

d)

Both, somehow

24.
This endothermic reaction is at equilibrium.
If its temperature is increased (at constant volume and pressure), which way will the equilibrium shift?
a)
To products (right)
b)
To reactants (left)
25.
In the Haber process, ammonia is made by reacting nitrogen with hydrogen at high temperature.
To maximise the yield of ammonia, what conditions should be used?
a)
High pressure
b)
Low pressure
26.

When extra NH3 is added to the following system at equilibrium:


3 H2(g) + N2(g) ⇌ 2 NH3(g)

a)

No change occurs

b)

In order to restore equilibrium, the reaction shifts right, toward products

c)

In order to restore equilibrium, the reaction shifts left, toward reactants

27.

When N2 is removed from the following system at equilibrium:

3 H2(g) + N2(g) ⇌ 2 NH3(g)

a)

No change occurs

b)

In order to restore equilibrium, the reaction shifts right, toward products

c)

In order to restore equilibrium, the reaction shifts left, toward reactants

28.

When H2 is added to the following system at equilibrium:

3 H2(g) + N2(g) ⇌ 2 NH3(g)

a)

No change occurs

b)

In order to restore equilibrium, the reaction shifts right, toward products

c)

In order to restore equilibrium, the reaction shifts left, toward reactants

29.

When the pressure is increased on the following system at equilibrium:

3 H2(g) + N2(g) ⇌ 2 NH3(g)

a)

No change occurs

b)

In order to restore equilibrium, the reaction shifts right, toward products

c)

In order to restore equilibrium, the reaction shifts left, toward reactants

30.

When the temperature is decreased on the following system at equilibrium:


2 HCl(aq) + Mg(s) ⇌ MgCl2(aq) + H2(g) + heat

a)

No change occurs

b)

In order to restore equilibrium, the reaction shifts right, toward products

c)

In order to restore equilibrium, the reaction shifts left, toward reactants

31.
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.
32.
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.
33.

2 SO2(g) + O2(g) ⇌ 2SO3(g) is an exothermic reaction.

What will happen if there is an increase temperature?

a)

shift equilibrium toward the right

b)

shift equilibrium toward the left

c)

increase pressure

d)

have no change

34.

4HCl (g) + O2 (g) ⇌ 2H2O (l) + 2Cl2 (g) + 113 kJ

Which of the following would drive the reaction to form more products?

a)

Increase in temperature

b)

Increase in pressure

c)

Increase in Cl2

d)

Decrease in HCl

35.

CH4 + 2H2S ↔ CS2 + 4H2+ heat

Which of the following would drive the reaction above to the right?

a)

Decrease in CH4

b)

increase in H2

c)

increase in temperature

d)

Decrease in temperature

36.

3 H2(g) + N2(g) ⇌ 2 NH3(g)


What will happen if there is an increase in NH3?

a)

shift equilibrium to the right, decreasing the concentration of H2

b)

shift equilibrium toward the right, increasing the concentration of N2

c)

shift equilibrium toward the left, increasing the concentration of H2

d)

shift equilibrium toward the left, decreasing the concentration of H2

37.

Which reaction will shift to the left when there is an increase in pressure?

a)

2H2 (g) + O2 (g) ↔ 2H2O (l)

b)

N2 (g) + 3H2 (g) ↔ 2NH3 (g)

c)

2Mg(s) + O2(g) ⇌ 2MgO(s)

d)

MgCO3(s) ⇌ MgO(s) + CO2(g)

38.

2SO2(g) + O2(g) ⇌ 2SO3(g)

Increasing volume of container will

a)

shift equilibrium right

b)

shift equilibrium left

c)

slow rate of reaction

d)

have no change

39.

2SO2(g) + O2(g) ⇌ 2SO3(g)

How does adding a catalyst affect this reaction?

a)

shifts equilibrium right

b)

shifts equilibrium left

c)

increases the rate of the reaction

40.
Why is equilibrium called a dynamic state?
a)
Chemists try to convert as much reactants as possible into products.
b)
The reactions at equilibrium continue to take place once equilibrium is established.
c)
The products of a forward reaction are favored, so equilibrium lies to the right.
d)
All chemical reactions are considered to be reversible under suitable conditions.
41.

What causes the reaction to favor the REVERSE reaction?

A + B ↔ C + D + energy

a)

Decreasing D

b)

Decreasing C

c)

Decreasing A

d)

Decreasing Temperature

42.

What causes the reaction to favor the FORWARD reaction?

A + B ↔ C + D + energy

a)

Increasing D

b)

Increasing C

c)

Increasing B

d)

Increasing Temperature

43.

The three factors that affect the equilibrium of a reaction are temperature, pressure and __________.

a)

catalysts

b)

concentration

c)

particle size

44.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
45.
During equilibrium, the rates of the forward and the reverse reaction are ________
a)
the same 
b)
unequal
c)
unequal for exothermic reactions
d)
unequal for endothermic reactions
46.
If a reaction is reversible and has reached equilibrium, what can be said about the amounts of reactants and products?
a)
some reactant, some product
b)
no reactant, all product
c)
all reactant, no product
47.
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.
48.
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.
49.
N2O4(g) ↔ 2 NO2(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 = [NO2]/[N2O4]2
50.
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]  
51.

Consider the following equilibrium:

2NO2(g) <-> N2O4(g)

A 1.00 L flask contains 0.030 mol NO2 and 0.040 mol N2O4 at equilibrium.

The value of Keq is

a)

0.023

b)

0.67

c)

1.3

d)

44

52.

Consider the following equilibrium:

PCl5(g) <-> PCl3(g) + Cl2(g)

A 1.00 L flask contains 0.0200 mol PCl5, 0.0500 mol PCl3 and 0.0500 mol Cl2 at

equilibrium. The value of Keq is

a)

0.125

b)

2.50

c)

5.00

d)

8.00

53.
What will happen when Qc is greater > than Kc?
a)
Equilibrium is disturbed
b)
Equilibrium contain more reactants than products
c)
Equilibrium will shift to the right to increase Qc
d)
Equilibrium will shift to the left to decrease Qc
54.
What will happen when Qc is less < than Kc?
a)
Equilibrium is disturbed
b)
Equilibrium contain more products than reactants
c)
Equilibrium will shift to the right to increase Qc
d)
Equilibrium will shift to the left to decrease Qc
55.

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])

56.
At equilibrium the concentration of all species in the reaction is _________.
a)
Constant
b)
Increasing
c)
Decreasing
d)
Oscillating
57.

What is happening in term of enthalpy?

KBr (s) → KBr (l)

a)

endothermic, +ΔH

b)

exothermic, +ΔH

c)

endothermic, -ΔH

d)

exothermic, -ΔH

58.

Water is boiled. What happens in terms of enthalpy?

a)

endothermic, +ΔH

b)

endothermic, -ΔH

c)

exothermic, +ΔH

d)

exothermic, -ΔH

59.
The following reaction :    
SO2 (g) +  NO2 (g) <=> SO3 (g) + NO (g)  
had reached a state of equilibrium, was found to contain  
0.40 mol L-1 SO3 , and 0.30 mol L-1 NO,
0.15 mol L-1NO2 , and 0.20 mol L-1 SO2.
Calculate the equilibrium constant  for this reaction. 
a)
4
b)
.42
c)
.25
d)
1
60.
An equilibrium constant with a large value, e.g. Kc = 1000, indicates…
a)
A very fast reaction
b)
Mostly products at equilibrium
c)
Mostly reactants at equilibrium
d)
Nothing useful at all

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