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Equilibrium and LeChatelier's Principle

Total questions: 27

Worksheet time: 48mins

Name
Class
Date
1.
For an endothermic reaction, heat can be thought of as:
a)
a reactant
b)
a product
c)
either it has no effect
d)
neither it effects both sides equally.
2.
For the reaction...
SO2 + O2  <−>  SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right 
d)
neither left nor right
3.
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
4.
For the reaction...
SO2 + O2 <−>  SO3
If the equilibrium shifts to the right, the concentration of SO3 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
5.
For the reaction...
SO2 + O2 <−>  SO3
If the concentration of O2 is decreased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right
d)
neither left nor right
6.
For the reaction...
SO2 + O2 <−>  SO3
If the equilibrium shifts to the left, the concentration of SO3 will ___________.
a)
increase
b)
decrease
c)
stay the same
d)
triple
7.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is added to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
left and right
d)
neither left nor right
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.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased,  which substance will increase in concentration?
a)
N2
b)
H2
c)
N2 and H2
d)
NH3
10.
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.
11.

For a chemical system at equilibrium, the concentrations of both the reactants and the products must

a)

decrease

b)

increase

c)

be constant

d)

be equal

12.

Which term identifies a factor that will shift a chemical equilibrium?

a)

Atomic Radius

b)

Catalyst

c)

Decay mode

d)

Temperature

13.

Given the equation representing a chemical reaction at equilibrium in a sealed, rigid container:

H2(g) + I2(g) + energy <--> 2HI(g)

When the concentration of H2(g) is increased by adding more hydrogen gas to the container at constant temperature, the equilibrium shifts

a)

to the right, and the concentration of HI(g) decreases

b)

to the right, and the concentration of HI(g) increases

c)

to the left, and the concentration of HI(g) decreases

14.
2.In the Haber process, gaseous ammonia is produced on an industrial scale by combining nitrogen and hydrogen gases, according to this equation: 
N2(g) + 3H2(g) ↔ 2NH3(g)
The process is exothermic. Which of the following actions will shift the reaction in the forward (product) direction?

a)
Decrease the pressure of the reaction.
b)
Increase the temperature of the reaction.
c)
Reduce ammonia concentration by removing ammonia from the reaction chamber.
d)
Reduce hydrogen concentration by reducing the amount of hydrogen in the reaction chamber.
15.
The principle that states that if a system at equilibrium is disturbed, the reaction will proceed in one direction or another in order to reestablish equilibrium, is known as:
a)
The principle of equilibrium
b)
Priestley’s principle
c)
Le Chatelier’s principle
d)
Faraday’s principle
16.
A system at equilibrium means it is still reacting.
a)
True
b)
False
17.
Increasing the pressure on the reaction:
2NO2 (g) ↔ N2O4 (g)
will:
a)
shift the reaction to the left towards the reactants, making more of the reactants.
b)
shift the equilibrium to the right towards the products, making more of the product.
c)
Have no effect on equilibrium.
18.
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
19.
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
20.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
21.
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.
22.
Which of the two graphs reaches equilibrium?
a)
The left one.
b)
The right one.
c)
Both of them.
d)
Neither.
23.

At what time (in seconds) is equilibrium established?

a)

0 seconds

b)

1 second

c)

5 seconds

d)

10 seconds

24.

A + B  <---->  AB The forward reaction forms the substance __________.

a)
A
b)
B
c)
AB
d)
A + B
25.

A + B  <---->  AB The forward reaction points towards the __________.

a)
left
b)
right
c)
up
d)
down
26.

A + B  <---->  AB The reverse reaction forms the substance __________.

a)
A
b)
B
c)
AB
d)
A + B
27.

A + B  <---->  AB The reverse reaction points towards the __________.

a)
left
b)
right
c)
up
d)
down

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