Chem 203 Equilibrium Systems Review: Acid-Base Focus for Chem 30 D1
Unit D—Chemical Equilibrium Focusing on Acid–
Base Systems
General Outcome 1:
Students will explain that there is a balance of opposing reactions in chemical
equilibrium systems
Knowledge
30–D1.1k Define equilibrium and state the criteria that apply to a chemical system in equilibrium;
i.e., closed system, constancy of properties, equal rates of forward and reverse reactions.
Which of the following statements applies to a system at equilibrium?
A. The rate of the forward reaction is equal to the rate of the reverse reaction.
B. The concentration of the reactants equals the concentration of the products.
C. The rate of the forward reaction is greater than the rate of the reverse reaction.
D. The concentration of the products is greater than the concentration of the reactants.
A
Which of the following properties would not be used to determine if the equilibrium system
represented by the equation above is at equilibrium?
A. Temperature
B. Pressure
C. Colour
D. Mass
D
Which of the following systems could be at equilibrium?
A. A closed bottle of carbonated water
B. A block of ice in a glass of water
C. Water boiling in a kettle
D. A glass of pop
A
Chem 203 Equilibrium Systems Review: Acid-Base Focus for Chem 30 D1
,Chem 203 Equilibrium Systems Review: Acid-Base Focus for Chem 30 D1
Knowledge
30–D1.2k Identify, write and interpret chemical equations for systems at equilibrium.
The equation that represents the equilibrium of phosphoric acid is
D
Knowledge
30–D1.3k Predict, qualitatively, using Le Châtelier’s principle, shifts in equilibrium caused by
changes in temperature, pressure, volume, concentration or the addition of a catalyst and describe
how these changes affect the equilibrium constant.
For the position of the equilibrium to shift toward the products, the pressure of the system should be
i by adjusting the volume of the closed system and the temperature should be ii .
The statement above is completed by the information in row
Row i ii
A. increased increased
B. increased decreased
C. decreased increased
D. decreased decreased
B
When a catalyst is added to this system at equilibrium, the position of the equilibrium i and the value
of ΔH° ii .
The statement above is completed by the information in row
Row i ii
A. shifts right increases
B. shifts right does not change
C. does not change increases
D. does not change does not change
D
Chem 203 Equilibrium Systems Review: Acid-Base Focus for Chem 30 D1
, Chem 203 Equilibrium Systems Review: Acid-Base Focus for Chem 30 D1
Use the following information to answer the next two questions.
Which of the following changes, when applied to this equilibrium system, would change the value of
the equilibrium constant?
A. An addition of a catalyst
B. An increase in temperature
C. An addition of hydrogen gas
D. A decrease in the volume of the flask
B
The empirical evidence that could be used to determine when this system reaches equilibrium is
A. colour
B. density
C. total mass
D. total pressure
A
When applied to an equilibrium system, which of the following stresses would cause a change in
the Kc value after the equilibrium has been re-established?
A. Addition of a catalyst
B. Decrease in temperature by cooling the system
C. Addition of an inert gas to increase the pressure
D. Decrease in concentration by removing a product
B
Chem 203 Equilibrium Systems Review: Acid-Base Focus for Chem 30 D1
Unit D—Chemical Equilibrium Focusing on Acid–
Base Systems
General Outcome 1:
Students will explain that there is a balance of opposing reactions in chemical
equilibrium systems
Knowledge
30–D1.1k Define equilibrium and state the criteria that apply to a chemical system in equilibrium;
i.e., closed system, constancy of properties, equal rates of forward and reverse reactions.
Which of the following statements applies to a system at equilibrium?
A. The rate of the forward reaction is equal to the rate of the reverse reaction.
B. The concentration of the reactants equals the concentration of the products.
C. The rate of the forward reaction is greater than the rate of the reverse reaction.
D. The concentration of the products is greater than the concentration of the reactants.
A
Which of the following properties would not be used to determine if the equilibrium system
represented by the equation above is at equilibrium?
A. Temperature
B. Pressure
C. Colour
D. Mass
D
Which of the following systems could be at equilibrium?
A. A closed bottle of carbonated water
B. A block of ice in a glass of water
C. Water boiling in a kettle
D. A glass of pop
A
Chem 203 Equilibrium Systems Review: Acid-Base Focus for Chem 30 D1
,Chem 203 Equilibrium Systems Review: Acid-Base Focus for Chem 30 D1
Knowledge
30–D1.2k Identify, write and interpret chemical equations for systems at equilibrium.
The equation that represents the equilibrium of phosphoric acid is
D
Knowledge
30–D1.3k Predict, qualitatively, using Le Châtelier’s principle, shifts in equilibrium caused by
changes in temperature, pressure, volume, concentration or the addition of a catalyst and describe
how these changes affect the equilibrium constant.
For the position of the equilibrium to shift toward the products, the pressure of the system should be
i by adjusting the volume of the closed system and the temperature should be ii .
The statement above is completed by the information in row
Row i ii
A. increased increased
B. increased decreased
C. decreased increased
D. decreased decreased
B
When a catalyst is added to this system at equilibrium, the position of the equilibrium i and the value
of ΔH° ii .
The statement above is completed by the information in row
Row i ii
A. shifts right increases
B. shifts right does not change
C. does not change increases
D. does not change does not change
D
Chem 203 Equilibrium Systems Review: Acid-Base Focus for Chem 30 D1
, Chem 203 Equilibrium Systems Review: Acid-Base Focus for Chem 30 D1
Use the following information to answer the next two questions.
Which of the following changes, when applied to this equilibrium system, would change the value of
the equilibrium constant?
A. An addition of a catalyst
B. An increase in temperature
C. An addition of hydrogen gas
D. A decrease in the volume of the flask
B
The empirical evidence that could be used to determine when this system reaches equilibrium is
A. colour
B. density
C. total mass
D. total pressure
A
When applied to an equilibrium system, which of the following stresses would cause a change in
the Kc value after the equilibrium has been re-established?
A. Addition of a catalyst
B. Decrease in temperature by cooling the system
C. Addition of an inert gas to increase the pressure
D. Decrease in concentration by removing a product
B
Chem 203 Equilibrium Systems Review: Acid-Base Focus for Chem 30 D1
