Q1. In a reversible reaction, if the concentration of products increases, what happens to the rate of the forward reaction? (2021)
Solution:
According to Le Chatelier's principle, if the concentration of products increases, the system will shift to the left, decreasing the rate of the forward reaction.
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Q2. For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens to the equilibrium if the volume of the container is decreased? (2022)
Solution:
Decreasing the volume increases the pressure, and according to Le Chatelier's principle, the equilibrium will shift towards the side with fewer moles of gas, which is the right side (2 moles of SO3).
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Q3. In a reversible reaction at equilibrium, what happens if the concentration of a reactant is increased? (2023)
Solution:
According to Le Chatelier's principle, increasing the concentration of a reactant will shift the equilibrium to the right to produce more products.
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Q4. In a reversible reaction, if the concentration of products increases, what happens to the equilibrium position? (2021)
Solution:
According to Le Chatelier's principle, if the concentration of products increases, the equilibrium will shift to the left to counteract the change.
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Q5. For the exothermic reaction A + B ⇌ C + heat, what will happen if the temperature is increased? (2020)
Solution:
For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants, as the system tries to absorb the added heat.
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Q6. In the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium position if the pressure is increased? (2023)
Solution:
Increasing the pressure shifts the equilibrium towards the side with fewer moles of gas, which in this case is the right side (2 moles of NH3).
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Q7. What is the equilibrium constant (Kc) for the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g)? (2022) 2022
Solution:
The equilibrium constant Kc for the formation of ammonia from nitrogen and hydrogen is typically around 1.0 × 10^5 at standard conditions.
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Q8. In a reversible reaction, if the concentration of products increases, what happens to the equilibrium position? (2021) 2021
Solution:
According to Le Chatelier's principle, if the concentration of products increases, the equilibrium will shift to the left to counteract the change.
⏱ Time: 0s
Q9. For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium if the volume of the container is decreased? (2020)
Solution:
Decreasing the volume increases the pressure, and according to Le Chatelier's principle, the equilibrium will shift to the side with fewer moles of gas, which is the right side in this case.
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Q10. In a reversible reaction at equilibrium, which of the following statements is true?
Solution:
At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction, which means the concentrations of reactants and products remain constant over time.
