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CHEMICAL EQUILIBRIA AND LE CHATELIER PRINCIPLE REVIEW

Total questions: 65

Worksheet time: 1hrs 16mins

Name
Class
Date
1.
What are the two factors to look for when determining if the reaction is at equilibrium?
a)
Forward reaction rate is faster than the reverse and concentrations are equal
b)
Forward and reverse reaction rates are equal and concentration is constant
c)
Forward and revers reaction rates are equal and concentration is equal
d)
Forward reaction rate is faster than the reverse and concentration is equal
2.
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
3.
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
4.
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
5.
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
6.
For the reaction...
energy +  N2(g)  +  O2(g)  <−>  2NO(g)
If  O2(g) is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
7.
For the reaction...
heat  +  N2(g)  +  O2(g)  <−>  2NO(g)
If the heat is removed to the chemical system, the equilibrium will _______.
a)
shift to the left
b)
shift to the right
c)
not shift
8.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased, the reaction will __________________.
a)
 shift to the left
b)
shift to the right
c)
not shift
9.
The three factors that affect the equilibrium of a reaction are temperature, pressure and __________. 
a)
energy
b)
concentration 
c)
enthalpy 
d)
ice 
10.
What would happen to the position of the equilibrium when Oxygen is added to the system?
 2SO3(g) ⇋ 2SO2(g) + O2(g) 
a)
SO3 will increase 
b)
SO3 will decrease 
c)
SO2 will increase
d)
none of the above
11.

What does Le Chatelier's Principle state about equilibrium?

a)

Le Chatelier's Principle only applies to gas reactions.

b)

The equilibrium remains unchanged regardless of external changes.

c)

The system will always shift to the right in response to any change.

d)

If a change is applied to a system at equilibrium, the system shifts to counteract that change.

12.

What effect does increasing temperature have on an exothermic reaction at equilibrium?

a)

The equilibrium shifts to the left, favoring reactants.

b)

The reaction rate decreases significantly with increased temperature.

c)

Temperature has no effect on the equilibrium position.

d)

The equilibrium shifts to the right, favoring products.

13.

Define dynamic equilibrium in the context of chemical reactions.

a)

Dynamic equilibrium is the state in a chemical reaction where the rates of the forward and reverse reactions are equal, leading to constant concentrations of reactants and products.

b)

Dynamic equilibrium is when the concentration of reactants is higher than that of products.

c)

Dynamic equilibrium is the point at which a reaction stops completely.

d)

Dynamic equilibrium occurs when all reactants are completely converted to products.

14.

How does a change in concentration affect the position of equilibrium?

a)

Increasing concentration always shifts equilibrium to the right.

b)

A change in concentration has no effect on equilibrium.

c)

A change in concentration shifts the equilibrium position to counteract the change.

d)

Decreasing concentration always shifts equilibrium to the left.

15.

What role do catalysts play in chemical equilibrium?

a)

Catalysts increase the rate of reaching equilibrium but do not affect the equilibrium position.

b)

Catalysts are consumed in the reaction and alter the final concentrations of reactants and products.

c)

Catalysts decrease the activation energy of the reaction but change the equilibrium constant.

d)

Catalysts shift the equilibrium position to favor products.

16.

What happens to the equilibrium if we add methane (CH4)?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

17.

What happens to the equilibrium if we remove water (H2O)?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

18.

What happens to the equilibrium if we remove heat?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

19.

What happens to the equilibrium if we add hydrogen (H2)?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

20.

What happens to the equilibrium if we remove carbon monoxide (CO)?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

21.

What happens when sodium ions (Na+) are added?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

There is no shift

22.

What happens when fluoride ions (Na+) are removed?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

There is no shift

23.

What happens when the system is cooled (heat is removed)?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

There is no shift

24.
For N2 + 3H2 →2NH3 . When pressure is increased the equilibrium shift to right. Why?
a)
To increase the amount of products
b)
To reduce the pressure, as right has less number of molecule
c)
Kc will increase when it is shifted to the right
d)
So it will increase the rate of reaction
25.
CoCI42- +6H2O →Co(H2O)62+ + 4CI- (ΔH = -ve) What will happen when temperature is increased?
a)
Position of equilibrium will shift to left
b)
Position of equilibrium will shift to right
c)
No change in position of equilibrium
d)
Equlibrium will not be affected
26.
For N2O4 → NO2 (ΔH = +ve). What will happen when temperature is increased?
a)
Position of equilibrium will shift to left
b)
Position of equilibrium will shift to right
c)
No change in position of equilibrium
d)
Equlibrium will not be affected
27.
N2O4 → NO2 (ΔH = +ve). Why when temperature is increased position of equilibrium is shifted to RIGHT?
a)
Forward reaction is endothermic, thus reducing the temp
b)
Forward reaction is exothermic, thus reducing the temp
c)
Forward reaction is endothermic, thus increasing the temp
d)
Forward reaction is exothermic, thus increasing the temp
28.
The following statement is true on the effect of increasing pressure EXCEPT
a)
Increase pressure increases the rate
b)
Increase pressure has no effect on rate constant
c)
Increase pressure has no effect on Kc
d)
Increase pressure has no effect on equilibrium composition.
29.
The following statement is true on the effect of increasing catalyst EXCEPT
a)
Increase catalyst increases the rate
b)
Increase catalyst has no effect on rate constant
c)
Increase catalyst has no effect on Kc
d)
Increase catalyst has no effect on equilibrium composition.
30.

What kind of equilibrium does the reaction below show?

H2(g) +I2(g) ↔ 2HI(g)

a)

Heterogeneous equilibrium, all the reactants and products are in the same physical state.

b)

Homogeneous equilibrium, all the reactants and products are in the same physical state.

c)

Heterogeneous equilibrium, the reactants and products are present in more than one physical state

d)

Homogeneous equilibrium, the reactants and products are present in more than one physical state

31.

What happens to the equilibrium if we add methane (CH4)?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

32.

What happens to the equilibrium if we remove water (H2O)?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

33.

What happens to the equilibrium if we remove heat?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

34.

What happens to the equilibrium if we add hydrogen (H2)?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

35.

What happens to the equilibrium if we remove carbon monoxide (CO)?

a)

It shifts left, towards the reactants

b)

It shifts right, towards the products

c)

It does not shift

36.

What happens when sodium ions (Na+) are added?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

There is no shift

37.

What happens when fluoride ions (Na+) are removed?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

There is no shift

38.

What happens when the system is cooled (heat is removed)?

a)

The reaction shifts left, towards the reactants

b)

The reaction shifts right, towards the products

c)

There is no shift

39.
For N2 + 3H2 →2NH3 . When pressure is increased the equilibrium shift to right. Why?
a)
To increase the amount of products
b)
To reduce the pressure, as right has less number of molecule
c)
Kc will increase when it is shifted to the right
d)
So it will increase the rate of reaction
40.
CoCI42- +6H2O →Co(H2O)62+ + 4CI- (ΔH = -ve) What will happen when temperature is increased?
a)
Position of equilibrium will shift to left
b)
Position of equilibrium will shift to right
c)
No change in position of equilibrium
d)
Equlibrium will not be affected
41.
For N2O4 → NO2 (ΔH = +ve). What will happen when temperature is increased?
a)
Position of equilibrium will shift to left
b)
Position of equilibrium will shift to right
c)
No change in position of equilibrium
d)
Equlibrium will not be affected
42.
N2O4 → NO2 (ΔH = +ve). Why when temperature is increased position of equilibrium is shifted to RIGHT?
a)
Forward reaction is endothermic, thus reducing the temp
b)
Forward reaction is exothermic, thus reducing the temp
c)
Forward reaction is endothermic, thus increasing the temp
d)
Forward reaction is exothermic, thus increasing the temp
43.
The following statement is true on the effect of increasing pressure EXCEPT
a)
Increase pressure increases the rate
b)
Increase pressure has no effect on rate constant
c)
Increase pressure has no effect on Kc
d)
Increase pressure has no effect on equilibrium composition.
44.
The following statement is true on the effect of increasing catalyst EXCEPT
a)
Increase catalyst increases the rate
b)
Increase catalyst has no effect on rate constant
c)
Increase catalyst has no effect on Kc
d)
Increase catalyst has no effect on equilibrium composition.
45.

What kind of equilibrium does the reaction below show?

H2(g) +I2(g) ↔ 2HI(g)

a)

Heterogeneous equilibrium, all the reactants and products are in the same physical state.

b)

Homogeneous equilibrium, all the reactants and products are in the same physical state.

c)

Heterogeneous equilibrium, the reactants and products are present in more than one physical state

d)

Homogeneous equilibrium, the reactants and products are present in more than one physical state

46.

What is Le Chatelier's principle and how does it relate to chemical equilibrium?

a)

Le Chatelier's principle is used to calculate the pH of a solution

b)

Le Chatelier's principle explains how a system at equilibrium responds to changes in conditions such as temperature, pressure, or concentration.

c)

Le Chatelier's principle only applies to solid-state reactions

d)

Le Chatelier's principle has no relation to chemical equilibrium

47.

Discuss the factors that can affect the equilibrium of a chemical reaction.

a)

Color of the reactants

b)

Size of the reaction vessel

c)

Time of day

d)

Concentration, temperature, pressure, and catalysts

48.

What is the effect of increasing the concentration of a reactant on the equilibrium position?

a)

No effect on the equilibrium position

b)

Causes the reaction to stop

c)

Shift to the right

d)

Shift to the left

49.

Explain the concept of dynamic equilibrium in chemical reactions.

a)

Equal rates of forward and reverse reactions

b)

The reaction only proceeds in one direction

c)

The reaction stops completely

d)

The reaction rate increases over time

50.

Which of the following factors does NOT affect the position of equilibrium in a chemical reaction?

a)

Temperature

b)

Pressure

c)

Catalyst

d)

Concentration

51.

If the concentration of a reactant is increased in a system at equilibrium, what will happen according to Le Chatelier's principle?

a)

The equilibrium will shift to the right.

b)

The equilibrium will shift to the left.

c)

The equilibrium will remain unchanged.

d)

The reaction will stop.

52.

Consider the reaction: N2(g)+3H2(g)⇌2NH3(g)N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) . What will happen to the equilibrium position if the pressure is increased?

a)

Shift to the right

b)

Shift to the left

c)

No change

d)

Reaction stops

53.

Explain why increasing the temperature of an exothermic reaction shifts the equilibrium to the left.

a)

Because it increases the concentration of reactants.

b)

Because it decreases the concentration of products.

c)

Because it favors the endothermic reverse reaction.

d)

Because it increases the rate of the forward reaction.

54.

For the reaction 2SO2(g)+O2(g)⇌2SO3(g)2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g) , what is the effect of adding more O2O_2 to the system at equilibrium?

a)

The equilibrium will shift to the right.

b)

The equilibrium will shift to the left.

c)

The equilibrium will remain unchanged.

d)

The reaction will stop.

55.

Describe how a catalyst affects the rate of a reaction and the position of equilibrium.

a)

Increases the rate of reaction and shifts equilibrium to the right.

b)

Increases the rate of reaction but does not affect the position of equilibrium.

c)

Decreases the rate of reaction and shifts equilibrium to the left.

d)

Decreases the rate of reaction but does not affect the position of equilibrium.

56.

In the reaction CO(g)+2H2(g)⇌CH3OH(g)CO(g) + 2H_2(g) \rightleftharpoons CH_3OH(g) , what will happen if the volume of the container is decreased?

a)

The equilibrium will shift to the right.

b)

The equilibrium will shift to the left.

c)

The equilibrium will remain unchanged.

d)

The reaction will stop.

57.

Predict the effect of decreasing temperature on the equilibrium position of an endothermic reaction.

a)

The equilibrium will shift to the right.

b)

The equilibrium will shift to the left.

c)

The equilibrium will remain unchanged.

d)

The reaction will stop.

58.

For the reaction 2NO2(g)⇌N2O4(g)2NO_2(g) \rightleftharpoons N_2O_4(g) , explain why increasing the pressure shifts the equilibrium to the right.

a)

Because it increases the concentration of NO2NO_2 .

b)

Because it decreases the concentration of N2O4N_2O_4 .

c)

Because it favors the formation of fewer gas molecules.

d)

Because it increases the rate of the forward reaction.

59.

What is the effect of adding a catalyst to a system at equilibrium?

a)

It shifts the equilibrium to the right.

b)

It shifts the equilibrium to the left.

c)

It increases the rate of both forward and reverse reactions equally.

d)

It stops the reaction.

60.

How does Le Chatelier's principle apply to the industrial synthesis of ammonia in the Haber process?

a)

By increasing temperature to shift equilibrium to the right.

b)

By increasing pressure to shift equilibrium to the right.

c)

By decreasing concentration of reactants to shift equilibrium to the right.

d)

By using a catalyst to shift equilibrium to the right.

61.

In the reaction H2(g)+Cl2(g)⇌2HCl(g)H_2(g) + Cl_2(g) \rightleftharpoons 2HCl(g) , what will happen if the concentration of HClHCl is decreased?

a)

The equilibrium will shift to the right.

b)

The equilibrium will shift to the left.

c)

The equilibrium will remain unchanged.

d)

The reaction will stop.

62.

An understanding of Le Chatelier’s principle is useful in the chemical industry. A prediction that can be made using this principle is the effect of...

a)

catalysts on the rate of reaction

b)

catalysts on the position of equilibrium

c)

changes in temperature on the rate of reaction

d)

changes in the concentration of reactants on the position of equilibrium

63.

How does the removal of a product from a system at dynamic equilibrium affect the position of equilibrium?

a)

It causes the reverse reaction to stop entirely.

b)

It favours the reverse reaction.

c)

It favours the forward reaction.

d)

It does not affect the position of equilibrium.

64.

Hydrogen is produced on an industrial scale from methane, as follows. If an inert gas is added to an equilibrium system at a constant temperature and a constant volume, the concentration of hydrogen will...

a)

increase.

b)

decrease.

c)

not change.

d)

decrease then increase.

65.

The temperature of an equilibrium system with an endothermic forward reaction is increased.

The value of K....

a)

will increase and the equilibrium position will shift to the right.

b)

will decrease and the equilibrium position will shift to the right

c)

will increase and the equilibrium position will shift to the left

d)

will decrease and the equilibrium position will shift to the left.

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