Q1. For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what is the expression for Kp? (2020)
Solution:
Kp is expressed in terms of partial pressures, so for the reaction, Kp = (P_NH3)^2 / (P_N2)(P_H2)^3.
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Q2. 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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Q3. In a reversible reaction at equilibrium, what happens if the temperature is increased? (2019)
Solution:
Increasing the temperature of an exothermic reaction shifts the equilibrium to the left (towards the reactants), while for an endothermic reaction, it shifts to the right (towards the products).
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Q4. In a reaction at equilibrium, if the concentration of reactants is increased, what will happen to the position of equilibrium? (2022)
Solution:
According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right to produce more products.
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Q5. In a reversible reaction, if the forward reaction is exothermic, what can be said about the reverse reaction? (2022)
Solution:
If the forward reaction is exothermic, the reverse reaction must be endothermic, as it absorbs heat.
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Q6. What is the effect of increasing pressure on the equilibrium of the reaction: 2N2(g) + 3H2(g) ⇌ 2NH3(g)? (2021)
Solution:
Increasing pressure shifts the equilibrium towards the side with fewer moles of gas. In this case, it shifts to the right, producing more NH3.
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Q7. In a reaction at equilibrium, if the temperature is increased for an exothermic reaction, what will happen? (2022)
Solution:
For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants.
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Q8. In a reversible reaction at equilibrium, if the concentration of reactants is increased, what will happen to the equilibrium position? (2023)
Solution:
According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products.
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Q9. In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if H2 is removed from the system, what will happen to the equilibrium? (2022)
Solution:
Removing H2 will shift the equilibrium to the left to produce more H2, according to Le Chatelier's principle.
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Q10. For the reaction: 2A(g) + B(g) ⇌ 3C(g), what is the correct expression for the equilibrium constant Kc? (2021)
Solution:
The equilibrium constant Kc is given by the expression Kc = [C]^3 / ([A]^2[B]), where the concentrations are raised to the power of their coefficients.
