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7E4 Equilibrium

Total questions: 26

Worksheet time: 25mins

Name
Class
Date
1.
The following factors affect the position of equilibrium EXCEPT
a)
Concentration
b)
Pressure
c)
Temperature
d)
States of matter
2.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Adding SO2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase rate of reaction

d)

have no change

3.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Increasing the temperature will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

4.

2SO2(g) + O2(g) ⇌ 2SO3(g) + Heat


Removing O2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

5.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Adding SO3(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase K

d)

have no change

6.

2SO2(g)+1O2(g) ⇌ 2SO3(g) + Heat


Increasing the volume of the container will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

slow rate of reaction

d)

have no change

7.

2SO2(g)+1O2(g) ⇌ 2SO3(g) + Heat


Increasing the pressure on the system will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

slow rate of reaction

d)

have no change

8.

2CrO42- + 2H+ → Cr2O72- + H2O


What will happen when H+ ions are added to the system?

a)

Position of equilibrium will shift to left and become more yellow

b)

Color of system will turn all yellow

c)

Color of system will turn all orange

d)

Equilibrium will shift to right and become more orange

9.

Heat + 1 N2O4 → 2 NO2


What will happen when the temperature is increased?

a)

Position of equilibrium will shift to left and become lighter in color

b)

Position of equilibrium will shift to right and become more brown

c)

No change in position of equilibrium

d)

Position of equilibrium will shift to right and become lighter in color

10.

2CrO42- + 2H+→Cr2O72- + H2O


What will happen when OH- ions are added to the system? HINT: They remove the H+ ions.

a)

Position of equilibrium will shift to right and become more orange

b)

Position of equilibrium will shift to left and become more yellow

c)

Position of equilibrium will shift to right and become more yellow

d)

OH- ions will not react, and thus no change is seen.

11.

Changes in pressure will only affect substances that are in the ______ state.

a)

solid

b)

gas

c)

liquid

12.
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
13.

Identify the incorrect statement about achieving equilibrium.

a)

achieved when product and reactant concentrations are equal

b)

achieved when forward and reverse reaction rates are same

c)

achieved when concentration of reactants is stable/constant

d)

achieved when concentration ratio of reactants to products becomes stable, thus fixing the equilibrium constant (equilibrium position)

14.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
15.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
16.
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]
17.

Le Chatelier's Principle states that if a chemical system at equilibrium is stressed,

a)

the system will adjust to increase the stress

b)

the system will adjust to reduce the stress

c)

the system will not adjust

18.
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
19.
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)
20.
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
21.
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
22.
Given: 2A(g) <=> 2B(g) + C(g). At a particular temperature, Kc = 16000.
Raising the pressure, by decreasing the volume of the container, will...
a)
cause the value of Kc to increase
b)
cause the value of Kc to decrease
c)
have no effect on the value of Kc as temperature does not change
d)
favour the forward reaction
23.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
24.
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
25.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If  NO is removed  from the system, the concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
26.
For the reaction...
H2 (g)  + Cl2 (g) <−>  2HCl (g)  +  heat
If the temperature is cooled, the _________ reaction will be favored.
a)
forward
b)
reverse
c)
forward and reverse

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