CHEM 104 Exam 7 Questions and
Answers Verified Solutions Latest Update
2026/2027
Question:
Which statement does NOT generally apply to a chemical rxn in dynamic equilibrium?
A. The rates of the forward & reverse rxns are equal
B. The concentration of the reactants and the products are constant
C. The concentration of the reactants and the products are equal
Answer:
C The reactants and the products concentrations do not need to be the same.
Question:
What is the equilibrium constant?
Answer:
The rate of equilibrium of concentration of products raised to their stoichiometric coefficients
divided by the concentrations of reactants raised to their stoichiometric coefficients.
Question:
What can a high K value represent? [ K > 1 ]
Answer:
Products dominant the reaction. Reaction is favored to the right.
Question:
What can a low K value represent? [ K < 1 ]
Answer:
Reactants dominant the reaction. Reaction is favored to the left.
,Question:
What can we tell about the chemical reaction just be looking at the K value?
Answer:
The magnitude of the equilibrium constant tells us whether a reaction favors products or reactants
at equilibrium.
Question:
What can you infer when the K constant is equal to 1?
Answer:
Comparable amounts of products and reactants are present at equilibrium.
Question:
The equilibrium constant for the reaction A (g) -> <- B (g) = 10. A reaction mixture initially
contains [A] = 1.1 M and [B] = 0.0 M. Which statement about this reaction is true at equilibrium?
A. The equilibrium reaction mixture contains [A] = 1.0 M and [B] = 0.1 M
B. The equilibrium reaction mixture contains [A] = 0.1 M and [B] = 1.0 M
C. The equilibrium reaction mixture contains equal concentrations of A and B.
Answer:
B because K = 10
Question:
If you reverse an equilibrium reaction, what do you do to the initial K value?
Answer:
Invert it. If K = 10 K now becomes 1/10
Question:
If you multiply the coefficients of an equilibrium reaction, what do you do to the initial K value?
Answer:
Raise the K to the same factor. If you multiplied by 2 Raise K to the 2 (K^2)
, Question:
If you add two or more reactions to obtain an overall one, what do you do to the initial K?
Answer:
Multiply the corresponding K constants by each other. K1 x K2
Question:
In what two ways can you write equilibrium constants?
Answer:
Kp and Kc
Question:
What is a Kc value?
Answer:
Equilibrium constant using concentrations
Question:
What is a Kp value?
Answer:
Equilibrium constant using partial pressures.
Question:
What must be true about the phases in the equilibrium reaction, to use a Kp?
Answer:
All must be in gaseous phases.
Question:
How do Kc and Kp relate?
Answer:
Answers Verified Solutions Latest Update
2026/2027
Question:
Which statement does NOT generally apply to a chemical rxn in dynamic equilibrium?
A. The rates of the forward & reverse rxns are equal
B. The concentration of the reactants and the products are constant
C. The concentration of the reactants and the products are equal
Answer:
C The reactants and the products concentrations do not need to be the same.
Question:
What is the equilibrium constant?
Answer:
The rate of equilibrium of concentration of products raised to their stoichiometric coefficients
divided by the concentrations of reactants raised to their stoichiometric coefficients.
Question:
What can a high K value represent? [ K > 1 ]
Answer:
Products dominant the reaction. Reaction is favored to the right.
Question:
What can a low K value represent? [ K < 1 ]
Answer:
Reactants dominant the reaction. Reaction is favored to the left.
,Question:
What can we tell about the chemical reaction just be looking at the K value?
Answer:
The magnitude of the equilibrium constant tells us whether a reaction favors products or reactants
at equilibrium.
Question:
What can you infer when the K constant is equal to 1?
Answer:
Comparable amounts of products and reactants are present at equilibrium.
Question:
The equilibrium constant for the reaction A (g) -> <- B (g) = 10. A reaction mixture initially
contains [A] = 1.1 M and [B] = 0.0 M. Which statement about this reaction is true at equilibrium?
A. The equilibrium reaction mixture contains [A] = 1.0 M and [B] = 0.1 M
B. The equilibrium reaction mixture contains [A] = 0.1 M and [B] = 1.0 M
C. The equilibrium reaction mixture contains equal concentrations of A and B.
Answer:
B because K = 10
Question:
If you reverse an equilibrium reaction, what do you do to the initial K value?
Answer:
Invert it. If K = 10 K now becomes 1/10
Question:
If you multiply the coefficients of an equilibrium reaction, what do you do to the initial K value?
Answer:
Raise the K to the same factor. If you multiplied by 2 Raise K to the 2 (K^2)
, Question:
If you add two or more reactions to obtain an overall one, what do you do to the initial K?
Answer:
Multiply the corresponding K constants by each other. K1 x K2
Question:
In what two ways can you write equilibrium constants?
Answer:
Kp and Kc
Question:
What is a Kc value?
Answer:
Equilibrium constant using concentrations
Question:
What is a Kp value?
Answer:
Equilibrium constant using partial pressures.
Question:
What must be true about the phases in the equilibrium reaction, to use a Kp?
Answer:
All must be in gaseous phases.
Question:
How do Kc and Kp relate?
Answer:
