CHEM134 C003 LESSON 6: ADVANCED
CHEMICAL EQUILIBRIUM QUESTIONS
AND ANSWERS WITH VERIFIED
SOLUTIONS 2026/2027 UPDATE. JUST
RELEASED
1. For the gaseous reaction 2SO2 + O2 ⇌ 2SO3, how does the value of Kp relate to Kc at 500
K?
A. Kp = Kc(RT)^1
B. Kp = Kc(RT)^-1
C. Kp = Kc(RT)^-2
D. Kp = Kc
Answer: B
Conceptual Explanation: The relationship is Kp = Kc(RT)^Δn. Here, Δn = (moles of
gaseous products) - (moles of gaseous reactants) = 2 - (2 + 1) = -1. Thus, Kp = Kc(RT)^-1.
2. In a system at equilibrium, what is the effect of adding a catalyst?
A. It increases the value of the equilibrium constant K.
,B. It shifts the equilibrium position toward the products.
C. It decreases the activation energy of only the forward reaction.
D. It increases the rate of both forward and reverse reactions equally.
Answer: D
Conceptual Explanation: A catalyst lowers the activation energy for both the forward and
reverse reactions equally, allowing equilibrium to be reached faster without changing the
equilibrium position or the value of K.
3. Given the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) with ΔH < 0, which change will increase the
yield of NH3?
A. Increasing the temperature
B. Decreasing the temperature
C. Increasing the volume of the container
D. Decreasing the pressure
Answer: B
Conceptual Explanation: Since the reaction is exothermic (ΔH < 0), decreasing the
temperature shifts the equilibrium toward the product side (right) to produce heat,
according to Le Chatelier’s principle.
, 4. If the reaction quotient Q is greater than the equilibrium constant K (Q > K), what must
happen for the system to reach equilibrium?
A. The reaction will proceed to the right.
B. The reaction will proceed to the left.
C. The concentration of products will increase.
D. The value of K will increase until it equals Q.
Answer: B
Conceptual Explanation: When Q > K, the ratio of products to reactants is higher than at
equilibrium. The system will shift to the left, consuming products and forming reactants
until Q = K.
5. Consider the heterogeneous equilibrium: CaCO3(s) ⇌ CaO(s) + CO2(g). What is the correct
expression for Kc?
A. Kc = [CO2]
B. Kc = [CaO][CO2] / [CaCO3]
C. Kc = 1 / [CO2]
D. Kc = [CaO] / [CaCO3]
Answer: A
CHEMICAL EQUILIBRIUM QUESTIONS
AND ANSWERS WITH VERIFIED
SOLUTIONS 2026/2027 UPDATE. JUST
RELEASED
1. For the gaseous reaction 2SO2 + O2 ⇌ 2SO3, how does the value of Kp relate to Kc at 500
K?
A. Kp = Kc(RT)^1
B. Kp = Kc(RT)^-1
C. Kp = Kc(RT)^-2
D. Kp = Kc
Answer: B
Conceptual Explanation: The relationship is Kp = Kc(RT)^Δn. Here, Δn = (moles of
gaseous products) - (moles of gaseous reactants) = 2 - (2 + 1) = -1. Thus, Kp = Kc(RT)^-1.
2. In a system at equilibrium, what is the effect of adding a catalyst?
A. It increases the value of the equilibrium constant K.
,B. It shifts the equilibrium position toward the products.
C. It decreases the activation energy of only the forward reaction.
D. It increases the rate of both forward and reverse reactions equally.
Answer: D
Conceptual Explanation: A catalyst lowers the activation energy for both the forward and
reverse reactions equally, allowing equilibrium to be reached faster without changing the
equilibrium position or the value of K.
3. Given the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) with ΔH < 0, which change will increase the
yield of NH3?
A. Increasing the temperature
B. Decreasing the temperature
C. Increasing the volume of the container
D. Decreasing the pressure
Answer: B
Conceptual Explanation: Since the reaction is exothermic (ΔH < 0), decreasing the
temperature shifts the equilibrium toward the product side (right) to produce heat,
according to Le Chatelier’s principle.
, 4. If the reaction quotient Q is greater than the equilibrium constant K (Q > K), what must
happen for the system to reach equilibrium?
A. The reaction will proceed to the right.
B. The reaction will proceed to the left.
C. The concentration of products will increase.
D. The value of K will increase until it equals Q.
Answer: B
Conceptual Explanation: When Q > K, the ratio of products to reactants is higher than at
equilibrium. The system will shift to the left, consuming products and forming reactants
until Q = K.
5. Consider the heterogeneous equilibrium: CaCO3(s) ⇌ CaO(s) + CO2(g). What is the correct
expression for Kc?
A. Kc = [CO2]
B. Kc = [CaO][CO2] / [CaCO3]
C. Kc = 1 / [CO2]
D. Kc = [CaO] / [CaCO3]
Answer: A
