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Which line in the table best describes the effect of adding a catalyst to the following reaction? 4NH₃(g) + 5O₂(g) ⇌ 4NO(g) + 6H₂O(g) ΔH = -ve Position of equilibrium | Rate of forward reaction A | unchanged | unchanged B | unchanged | increased C | moves to right | unchanged D | moves to right | increased - Scottish Highers Chemistry - Question 20 - 2017
Question 20
Which line in the table best describes the effect of adding a catalyst to the following reaction? 4NH₃(g) + 5O₂(g) ⇌ 4NO(g) + 6H₂O(g) ΔH = -ve Position of equilib... show full transcript
Worked Solution & Example Answer:Which line in the table best describes the effect of adding a catalyst to the following reaction? 4NH₃(g) + 5O₂(g) ⇌ 4NO(g) + 6H₂O(g) ΔH = -ve Position of equilibrium | Rate of forward reaction A | unchanged | unchanged B | unchanged | increased C | moves to right | unchanged D | moves to right | increased - Scottish Highers Chemistry - Question 20 - 2017
Step 1
Which line in the table best describes the effect of adding a catalyst to the following reaction?
Answer
When a catalyst is added to a reaction, it lowers the activation energy, allowing the reaction to reach equilibrium faster.
However, it does not alter the position of the equilibrium. This means that while the rate of the forward reaction will increase, the position of the equilibrium will remain unchanged.
Given the options presented:
- Option A indicates both position and rate remain unchanged, which is incorrect.
- Option B states the position is unchanged and the rate increases, which is the correct answer.
- Option C suggests the position moves to the right with an unchanged rate, which is incorrect.
- Option D proposes both an increase in rate and a shift in position, which is also incorrect.
Thus, the correct line is B: 'unchanged' for position and 'increased' for the rate of forward reaction.