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CHEMICAL EQUILIBRIUM

Total questions: 18

Worksheet time: 5hrs 30mins

Name
Class
Date
1.

Calculate the equilibrium constant (Kc) for the given reaction and tell whether equilibrium lies to the left or the right.

PCl5 (g) ↔ PCl3 (g) + Cl2 (g)

Equilibrium concentrations are: [PCl5] = 0.25 M, [PCl3] = 9.7 × 10-4 M, and [Cl2] = 3.2 × 10-3 M.

a)

1.02 lies to the left

b)

0.000012 lies to the left

c)

1.02 lies to the right

d)

0.000012416 lies to the left

2.
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]
3.

When 0.40 mole of SO2 and 0.60 mole of O2 are placed in an evacuated 1.00–liter flask, the reaction represented below occurs.

2SO2 (g) + O2 (g) ↔ 2SO3 (g)

After the reactants and the product reach equilibrium and the initial temperature is restored, the flask is found to contain 0.30 mole of SO3. Based on these results, the equilibrium constant, Kc, for the reaction is

a)

20

b)

10

c)

6.7

d)

2.0

4.

H2(g)+Cl2(g)⇌2HCl(g)

The forward reaction is exothermic. What will happen to the equilibrium if the temperature is increased?

a)

equilibrium shifts right

b)

equilibrium shifts left

c)

You cannot predict the effect

d)

no change

5.

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]
6.
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 conctant
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
7.

Predict whether the reaction will shift to the right, left or not be affected by an INCREASE in temperature

2H2O2 (g) ↔ 2H2O (g) + O2 (g) exothermic

a)

left

b)

right

c)

no effect

8.
2SO2(g)+O2(g)⇌2SO3(g)
Removing O2(g) will
a)
shift equilibrium right
b)
shift equilibrium left
c)
increase pressure
d)
have no change
9.

Consider the following system at equilibrium:

CH4(g) + 2H2O (g) ↔ CO2 (g) + 4H2O (g)

Suppose the concentration of CH4 decreased, in which direction does the reaction shift to reestablish equilibrium?

a)

The reaction shifts to the left

b)

The reaction shifts to the right

10.

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)
11.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
12.
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
13.

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
14.
dynamic equilibrium
a)
condition of continuous, random movement of particles but no overall change in concentration of materials
b)
the process by which one or more substances change to produce one or more different substances
c)
a condition where the reaction occurring in a system is completely halted and there exists no movement between the reactants and the products corresponding to the chemical reaction
d)
a substance that takes part in and undergoes change in a chemical reaction
15.
static equilibrium
a)
condition of continuous, random movement of particles but no overall change in concentration of materials
b)
the reaction that forms reactants from products
c)
a condition where the reaction occurring in a system is completely halted and there exists no movement between the reactants and the products corresponding to the chemical reaction
d)
a measurement of how much solute exists within a certain volume of solvent or solution
16.

For the graph, choose the CORRECT statement.

a)

The rate of reaction slowly increase

b)

The systems never reach equilibrium

c)

At equilibrium, more NO2 is present than N2O4.

d)

At start of reaction, only NO2 was present.

17.

For the reaction, choose the CORRECT equilibrium constant, Kc.

a)
b)
c)
d)
18.

What is the Kc expression for the reaction below:
SOCl2(g)  +  H2O(g)   ⇌    SO2(g)  +  2HCl(g)

a)

[SO2][2HCl][SOCl2][H2O]\frac{[SO_2][2HCl]}{[SOCl_2][H_2O]}  

b)

[SO2][HCl]2[SOCl2][H2O]\frac{[SO_2][HCl]^2}{[SOCl_2][H_2O]}  

c)

[SOCl2][H2O][SO2][2HCl]\frac{[SOCl_2][H_2O]}{[SO_2][2HCl]}  

d)

[SOCl2][H2O][[SO2][2HCl]\frac{[SOCl_2][H_2O]}{\left[[SO_2\right][2HCl]}  

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