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General Principles of Chemical Equilibrium

Total questions: 20

Worksheet time: 13mins

Name
Class
Date
1.

What type of reactions can able to change products back to the their original form?

a)

Reversible reactions

b)

Irreversible reactions

c)

Combustion reactions

d)

Combination reactions

2.

If a reversible reaction is exothermic in the forward direction, it will be ...

a)

exothermic in the reverse direction

b)

endothermic in the forward direction too

c)

endothermic in the reverse direction

d)

not involve energy in reverse direction

3.

Why is a reaction described as irreversible?

a)

The products cannot be turned directly back into the reactants.

b)

You need to apply heat to make the reaction work.

c)

The products can be turned back into the reactants.

d)

The reactants cannot be turned into the products.

4.

Which of the following reactions never goes completion in a closed container?

a)

H2 + I2 ⇌ 2HI

b)

C2H5OH + 3O2 → 2CO2 + 3H2O

c)

NaOH + HCl → NaCl + H2O

d)

CuSO4 + Zn → ZnSO4 + Cu

5.

What is a closed system

a)

It gives out energy

b)

The reactants and the products do not escape from reaction mixture

c)

It takes in energy

d)

The reactants and the products escape from he reaction mixture to be kept in the system

6.

What is equal during chemical equilibrium?

a)

the forward & reverse rates of reaction in a closed system

b)

the concentration or pressure of reactants & products

c)

the amount of activation energy (Ea) in both directions of the chemical change

d)

the forward & reverse rates of reaction in an open system

7.
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.
8.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
9.
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
10.

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 reaction rate and amounts of reactants are greater than the products

b)

Forward and reverse reaction rates are equal and amounts of reactants and products are constant

c)

Forward reaction rate is slower than the reverse reaction rate and amounts of reactants are greater than the products

d)

Forward reaction rate is faster than the reverse reaction rate and amounts of products are greater than the reactants

11.
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]
12.
When K is large, 
a)
There are more products than reactants when the reaction reached equilibrium.
b)
There are more reactant than products when the reaction reached equilibrium.
c)
The amount of reactants is equal to the amount of products.
13.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
14.

What is the Keq expression for this reaction?

2 NO(g) + O2(g) ⇌ 2 NO2(g)

a)

Keq = [NO2]2 / [NO]2 [O2]

b)

Keq = [NO]2 [O2] / [NO2]2

c)

Keq = [NO]2 [O2] [NO2]2

d)

Keq = [NO2]2 / [NO]2 + [O2]

15.

When all reactants and products have the same physical state, then the reaction is called

a)

Heterogeneous equilibrium

b)

Homogeneous equilibrium

16.

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]}  

17.

Which of the following chemical reactions is reversible?

a)

CH4 + O2 ⇌ CO2 + H2O

b)

CuSO4.5H2O → CuSO4 + 5H2O

c)

NH4Cl ⇌ NH3 + HCl

d)

CaCO3 → CaO +CO2

18.

What is dynamic equilibrium?

a)

The reaction goes forward

b)

The reaction goes backward

c)

The rate of forward and backward reaction is equal

d)

The equilibrium is dynamite

19.
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.
20.
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.

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