Photo AI
Consider the following system which is at equilibrium in a rigid, sealed container - HSC - SSCE Chemistry - Question 23 - 2022 - Paper 1
Question 23
Consider the following system which is at equilibrium in a rigid, sealed container. $$4 ext{NH}_3(g) + 5 ext{O}_2(g) ightleftharpoons 4 ext{NO}(g) + 6 ext{H}_2... show full transcript
Worked Solution & Example Answer:Consider the following system which is at equilibrium in a rigid, sealed container - HSC - SSCE Chemistry - Question 23 - 2022 - Paper 1
Step 1
Identify what would happen to the amount of NO(g) if the temperature was increased.
Answer
Increasing the temperature will shift the equilibrium position of the reaction. Since the reaction has a negative enthalpy change (), it is exothermic. According to Le Chatelier's principle, increasing the temperature favors the endothermic direction. Therefore, the amount of NO(g) will decrease as the reaction shifts to the left.
Step 2
Explain why a catalyst does not affect the equilibrium position of this system.
Answer
A catalyst speeds up both the forward and reverse reactions equally by providing an alternative reaction pathway with a lower activation energy. However, since it affects both directions equally, the equilibrium position remains unchanged. The rates of reaction increase, but the concentrations of reactants and products at equilibrium do not change.
Step 3
Using collision theory, explain what would happen to the concentration of NO(g) if H2O(g) was removed from the system.
Answer
When H2O(g) is removed, the concentration of H2O decreases, which affects reaction dynamics. According to collision theory, lowering the concentration of products (H2O) shifts the equilibrium to the right to produce more of it. Consequently, the concentration of NO(g) will increase as the system works to restore equilibrium by favoring the forward reaction.