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Equilibrium

Total questions: 35

Worksheet time: 48mins

Name
Class
Date
1.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Neutralise the reaction
d)
increase collision between the particles thus increasing the rate.
2.
B represents
a)
energy absorbed
b)
energy released
c)
activation energy
3.

A chemical reaction that requires energy to happen

a)

Exothermic

b)

Endothermic

c)

Explosive

d)

Hot reaction

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.
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.
7.

N2O4(g) ↔ 2 NO2(g)

What is the concentration equilibrium constant expression?

a)

Keq = [NO2]2/[N2O4]

b)

Keq = [N2O4]/[NO2]2

c)

Keq = [N2O4]2/[NO2]

d)

Keq = [NO2]/[N2O4]2

8.
What is the equilibrium-constant expression for 
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
a)
Kc= [CO][H2O] / [CO2][H2]  
b)
Kc= [CO2][H2] / [CO]
c)
Kc= [CO2][H2] / [CO][H2O]
d)
Kc= [CO] / [CO2][H2]  
9.
What is the equilibrium expression for:
Fe3O4(s) + 4H2(g) <--> 3Fe(s) + 4H2O(g)
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])
10.
Why does increased concentration increase the rate of reaction?
a)
the activation energy is lowered
b)
collisions occur with greater energy
c)
the frequency of collisions is increased
11.

CO (g) + 3H2 (g) <----> CH4 (g) + 3H2O (g) At equilibrium [CO] = 4.0 M. [H2] = 2.8 M. [CH4] = .75 M, and [H2O] = .12M. Find the Keq constant.

a)

Keq =1.65 x 104

b)

Keq = 6.5 x 10-6

c)

Keq = 1.48 x 10-5

d)

Keq = 3.2 x 105

12.
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
13.
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
14.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is removed from the chemical system, the concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
15.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is added to the chemical system, the concentration of O2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
triple
16.

For the following hypothetical equilibrium, what is the value of the equilibrium constant if the concentration are as shown?

A (g) + 2B (g) <-----> C (g)

[A] = 0.000045 M, [B] = 0.022 M, [C] = 0.0094 M

Calculate Keq:

a)

.22

b)

9.9

c)

4.3 x 105

d)

2.3 x 108

17.

For the reaction SO2(g) + NO2(g) <-> SO3(g) + NO(g), the equilibrium constant is 18.0 at 1,200ºC. If 0.05 M of SO2 and 0.10 M NO2 are placed in a container, what concentration of SO3 will be present at equilibrium?

a)

0.11 M

b)

0.95 M

c)

0.30M

d)

2.22 M

18.

What is the Keq expression for the following 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 = 2[NO][O2] / 2[NO2]

19.
Initially, 0.84 moles of PCl5(g) is placed in a 1.0L flask.  At equilibrium, 0.72 moles of PCl5(g) is present.  What is the value of Kc for this reaction?
PCl5(g) ↔ PCl3(g) + Cl2(g)
a)
0.62
b)
0.020
c)
0.72
d)
0.12
20.
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.
21.
Le Chatelier's Principle states that.... 
If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium................
a)
moves to increase the change
b)
moves to counteract the change
c)
does not change
22.

The following reaction :

SO2 (g) + NO2 (g) <=> SO3 (g) + NO (g)

had reached a state of equilibrium, was found to contain

0.40 M SO3 , and 0.30 M NO, 0.15 M NO2 , and 0.20 M SO2.

Calculate the equilibrium constant for this reaction.

a)

4

b)

.42

c)

.25

d)

1

23.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
24.
Keq < 1
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.
25.
When Keq > 1, 
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.
26.
Which of the two graphs reaches equilibrium?
a)
The left one.
b)
The right one.
c)
Both of them.
d)
Neither.
27.
A substance that increases speed of chemical reaction without being being changed is called:
a)
Catalyst
b)
Acid
c)
Base
d)
pressure
28.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
29.
Increasing the concentration increases the speed of reaction by
a)
lowering activation energy
b)
increasing collisions
c)
speeding up the reactants
d)
exposing more reactant
30.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
31.
Which of the following slows down the rate of a chemical reaction?
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
32.

Q21. Determine the value of K for the reaction:

2 N2(g) + O2(g) ⇄ 2 N2O(g)

Equilibrium concentrations are:

[N2] = 3.6 M, [O2] = 4.1 M,

[N2O] = 3.3 × 10-18 M

a)

2.0 × 10-37

b)

4.5 × 1018

c)

5.0 × 1036

d)

2.2 × 10-19

33.
What is the activation energy?
a)
the quantity of heat absorbed in a reaction
b)
the minimum energy needed to begin a reaction
c)
the energy given off after reactants collide.
d)
both the energy and frequeny of collisions in increased
the energy difference between reactants and products
34.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
35.
A mixture of 0.500 mol H2 and 0.500 mol I2 was placed in a 1.00L flask.  The equilibrium constant Keq for the reaction H2(g) + I2(g) ↔ 2HI(g) is 54.3.  What is the concentration of HI at equilibrium?
a)
0.5M
b)
1.0M
c)
0.786M
d)
3.7M

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