WorksheetsEquilibrium
Total questions: 20
Worksheet time: 18mins
Name
Class
Date
1.
Given the equation representing a reaction at equilibrium:
N2(g) + 3H2(g) --> 2NH3(g) + energy
Which change causes the equilibrium to shift to the right?
N2(g) + 3H2(g) --> 2NH3(g) + energy
Which change causes the equilibrium to shift to the right?
a)
decreasing the concentration of H2(g)
b)
decreasing the pressure
c)
increasing the concentration of N2(g)
d)
increasing the temperature
2.
Given the reaction at equilibrium:
A(g) + B(g) <=> A2B3(g)
Which change will not affect the equilibrium concentrations of A(g), B(g), and A2B3(g)?
A(g) + B(g) <=> A2B3(g)
Which change will not affect the equilibrium concentrations of A(g), B(g), and A2B3(g)?
a)
adding more A(g)
b)
adding a catalyst
c)
increasing the temperature
d)
increasing the pressure
3.
Ammonia is produced commercially by the Haber reaction: N2 (g) + 3 H2 (g) --> 2 NH3 (g)
The formation of ammonia is favored by
The formation of ammonia is favored by
a)
an increase in pressure
b)
a decrease in pressure
c)
removal of N2(g)
d)
removal of H2(g)
4.
Given the reaction at equilibrium:
2H2(g) + O2(g) ↔ 2H2O(g) + energy
Which concentration changes occur when the temperature of the system is increased?
2H2(g) + O2(g) ↔ 2H2O(g) + energy
Which concentration changes occur when the temperature of the system is increased?
a)
The [H2] decreases and the [O2] decreases.
b)
The [H2] decreases and the [O2] increases.
c)
The [H2] increases and the [O2] decreases.
d)
The [H2] increases and the [O2] increases.
5.
Given the reaction at equilibrium:
AgCl(s) ↔ Ag+(aq) + Cl-(aq)
The addition of Cl- ions will cause the concentration of Ag+(aq) to
AgCl(s) ↔ Ag+(aq) + Cl-(aq)
The addition of Cl- ions will cause the concentration of Ag+(aq) to
a)
decrease as the amount of AgCl(s) decreases
b)
decrease as the amount of AgCl(s) increases
c)
increase as the amount of AgCl(s) decreases
d)
increase as the amount of AgCl(s) increases
6.
Which statement is true for a saturated solution?
a)
It must be a concentrated solution.
b)
It must be a diluted solution.
c)
Neither dissolving nor crystallizing is occurring.
d)
The rate of dissolving equals the rate of crystallizing.
7.
In which reaction at equilibrium will the point of equilibrium shift to the right when the pressure decreases at constant temperature?
a)
N2(g) + 3H2(g) ↔ 2NH3(g)
b)
H2(g) + Br2(g) ↔ 2HBr(g)
c)
CaCO3(s) ↔ CaO(s) + CO2(g)
d)
N2(g) + O2(g) ↔ 2NO(g)
8.
Given the reaction at equilibrium:
N2(g) + 3H2(g) ↔ 2NH3(g)
Increasing the concentration of N2(g) will increase the forward reaction rate due to
N2(g) + 3H2(g) ↔ 2NH3(g)
Increasing the concentration of N2(g) will increase the forward reaction rate due to
a)
a decrease in the number of effective collisions
b)
an increase in the number of effective collisions
c)
a decrease in the activation energy
d)
an increase in the activation energy
9.
Given the reaction at equilibrium:
N2(g) + O2(g) ↔ 2NO(g)
As the concentration of N2(g) is increased, the concentration of O2(g) will
N2(g) + O2(g) ↔ 2NO(g)
As the concentration of N2(g) is increased, the concentration of O2(g) will
a)
decrease
b)
increase
c)
remain the same
10.
Given the reaction system in a closed container at equilibrium and at a temperature of 298 K:
N2O4 (g) <--> 2NO2 (g)
The measurable quantities of the gases at equilibrium must be
N2O4 (g) <--> 2NO2 (g)
The measurable quantities of the gases at equilibrium must be
a)
decreasing
b)
increasing
c)
equal
d)
constant
11.
What conditions that must be met in order for a chemical reaction to take place?
a)
Collisions with the proper orientation
b)
Sufficient activation energy
c)
Appropriate coefficient of friction
d)
Both collisions with the proper orientation and sufficient energy
12.
Which is a factor that would not affect the rate of a reaction?
a)
Temperature
b)
Adding a catalyst
c)
Concentration
d)
The weather
13.
What factor can be increased to provide more collisions for gases only?
a)
Temperature
b)
Surface area
c)
Pressure
d)
Adding a catalyst
14.
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.
15.
At what time (in seconds) is equilibrium established?
a)
0 seconds
b)
1 second
c)
5 seconds
d)
10 seconds
16.
Why is equilibrium called a dynamic state?
a)
Chemists try to convert as much reactants as possible into products.
b)
The reactions at equilibrium continue to take place once equilibrium is established.
c)
The products of a forward reaction are favored, so equilibrium lies to the right.
d)
All chemical reactions are considered to be reversible under suitable conditions.
17.
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.
18.
Consider the following equilibrium system:
CaCO3(s) ⇄ CaO(s) + CO2(g)
Which one of the following changes would cause the above system to shift left?
CaCO3(s) ⇄ CaO(s) + CO2(g)
Which one of the following changes would cause the above system to shift left?
a)
Add more CaO
b)
Remove CO2
c)
Add more CaCO3
d)
Add a catalyst
19.
An exothermic reaction is allowed to reach equilibrium. If heat energy is then removed, the equilibrium will shift
a)
Toward the middle
b)
Toward the reactant side
c)
Toward the product side
d)
The reaction will not shift
20.
What happened at point t1?
a)
NH3 was added
b)
H2 was added
c)
N2 was added
d)
Temperature was increased
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