Q1. For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what is the expression for the equilibrium constant Kp? (2020)
Solution:
Kp is expressed in terms of the partial pressures of the gases involved in the reaction. For this reaction, Kp = (P_NH3)^2 / (P_N2)(P_H2)^3.
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Q2. In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what is the effect of increasing the concentration of CO? (2023)
Solution:
Increasing the concentration of CO will shift the equilibrium to the right, favoring the formation of CH3OH.
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Q3. In a reaction at equilibrium, if the concentration of a reactant is increased, what will happen to the equilibrium position? (2019)
Solution:
Increasing the concentration of a reactant will shift the equilibrium position to the right, favoring the formation of products.
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Q4. For the reaction: 2A(g) + B(g) ⇌ 3C(g), if the volume of the container is decreased, what will be the effect on the equilibrium? (2022)
Solution:
Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas. Here, it shifts to the right, producing more C.
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Q5. In a reaction at equilibrium, if the concentration of reactants is increased, what will happen? (2022)
Solution:
According to Le Chatelier's principle, if the concentration of reactants is increased, the equilibrium will shift to the right to produce more products.
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Q6. What happens to the equilibrium constant when a reaction is multiplied by a factor? (2023)
Solution:
When a balanced equation is multiplied by a factor, the equilibrium constant is raised to the power of that factor.
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Q7. The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 4. What is the value of Kp? (2023)
Solution:
Kp can be calculated from Kc using the relation Kp = Kc(RT)^(Δn), where Δn is the change in moles of gas. Here, Δn = 2 - 3 = -1, so Kp = Kc(0.0821T)^(-1). Assuming standard conditions, Kp = 4 * (1/RT) = 16.
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Q8. What is the effect of increasing the temperature on the equilibrium constant Kc for an endothermic reaction? (2023)
Solution:
For an endothermic reaction, increasing the temperature shifts the equilibrium to the right, thus increasing the value of Kc.
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Q9. Which of the following changes will shift the equilibrium to the right for the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g)? (2022)
Solution:
According to Le Chatelier's principle, increasing the concentration of a reactant (O2 in this case) will shift the equilibrium to the right, favoring the formation of products.
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Q10. If the equilibrium constant Kc for a reaction is 10, what is the value of Kc for the reverse reaction? (2020)
Solution:
For the reverse reaction, Kc is the reciprocal of the forward reaction. Therefore, Kc (reverse) = 1/Kc (forward) = 1/10 = 0.1.
