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Chemical Equilibrium

Total questions: 25

Worksheet time: 16mins

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

Which chemical species 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
3.

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.
4.

Dedcue at what time the reaction reached equilibrium?

a)
t1
b)
t2
c)
t3
d)
t4
5.

For the reaction... SO2 + O2  ⇌ SO3 If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.

a)
to the left
b)
to the right
c)
to the left and right 
d)
neither left nor right
6.

For the reaction... SO2 + O2 ⇌ SO3 If the equilibrium position shifts to the right, the concentration of O2 will ___________.

a)
increase
b)
decrease
c)
remain the same
d)
double
7.

For the reaction... N2  +  O2  ⇌  2NO If  O2 is removed, the  concentration of N2 will _______.

a)
increase
b)
decrease
c)
remain the same
d)
double
8.

For the reaction... N2 (g) +  3 H2 (g) ⇌ 2 NH3 (g) If the pressure in the system is increased,  which substance(s) will increase in concentration?

a)
N2  (as 2 mol gas  → 4 mol gas)
b)
H2 (as 2 mol gas  → 4 mol gas)
c)
N2 and H2 (as 2 mol gas  → 4 mol gas)
d)
NH3 (as 4 mol gas  → 2 mol gas)
9.
What is the Kc expression for this reaction?
   2 NO(g)  +  O2(g) ⇌  2 NO2(g)
a)
Kc = [NO2]2 / [NO]2 [O2]
b)
Kc =  [NO]2 [O2] / [NO2]2
c)
Kc = [NO]2 [O2] [NO2]2
d)
Kc = [NO2]2 / [NO]2 +  [O2]
10.

For the reaction... N2  +  O2  ⇌  2NO:  Δ H = +182 kJ mol-1. If the temperature is increased the equilibrium position will shift _______.

a)
to the left
b)
to the right
c)
to the left and right
d)
neither left nor right
11.

Consider the following reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g):  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
12.
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
13.

Le Chatelier's Principle states that "If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium __________"

a)

shifts to increase the change

b)

shifts to counteract the change

c)
does not change
14.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
15.

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
16.

For the reaction... H2 (g)  + Cl2 (g)  ⇌  2HCl (g)  +  heat If the pressure in the system is increased, the equilibrium position will _______.

a)
shift to the left
b)
shift to the right
c)
not shift position at all as 2 mol gas <=> 2 mol gas
17.

What is the equilibrium expression for: Fe3O4(s) + 4H2(g) ⇌ 3Fe(s) + 4H2O(g) Kc =

a)
[Fe]3 [H2O]4  / [Fe3O4] [H2]4
b)
[Fe3O4] [H2]4 /  [Fe]3 [H2O]4
c)
[H2O]4 / [H2]4
d)
[Fe] [H2O] / [Fe3O4] [H2]
18.

Around what time does the reaction reach equilibrium?

a)

25 min

b)

70 min

c)

45 min

d)

80 min

19.

Which of the two graphs reaches equilibrium?

a)

Neither

b)

The left

c)

Both

d)

The right

20.

Which of the following is NOT true at equilibrium?

a)

The concentrations of reactants and products do not change.

b)

The forward and reverse reactions proceed at the same rate.

c)

The concentration of the reactants is equal to the concentration of the products.

d)

The forward and reverse reactions continue to occur.

21.

Deduce the stress that occurred at 10 minutes

a)

Temperature change

b)

Increase in pressure

c)

CO was removed

d)

CO was added

22.

Deduce the stress that occurred at 14 minutes

a)

Decrease in pressure

b)

Increase in pressure

c)

Temperature change

d)

A catalyst was added

23.

Deduce the stress that occurred at 4 minutes (note this reaction is endothermic)

a)

No stress - the system is at equilibrium

b)

Increase in pressure

c)

Temperature decreased

d)

Temperature increased

24.

A chemcial system is said to be at equilibrium when:

a)

Qc = Kc

b)

Qc >>   Kc

c)

Qc <<   Kc

d)

Qc + Kc = 1

25.

Dynamic, chemical equilibrium can only occur in a/an

a)

Open System

b)

Closed System

c)

Either open or closed

d)

Neither open or closed

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