Consider the reaction: 2A\(_{(g)}\) \(\Leftrightarrow\) B\(_{(g)}\) + C\(_{(g)}\) \(\Delta\)H = +25.6 kJ. Which of the...
Consider the reaction:
2A\(_{(g)}\) \(\Leftrightarrow\) B\(_{(g)}\) + C\(_{(g)}\) \(\Delta\)H = +25.6 kJ.
Which of the following changes will favour the formation of the products of the reaction represented above, at equilibrium?
- A) decrease in temperature
- B) increase in pressure
- C) increase in temperature
- D) decrease in volume
Correct Answer: C) increase in temperature
Explanation
The given reaction is:
2A(g) ? B(g) + C(g) with ?H = +25.6 kJ.
Since ?H is positive, the reaction is endothermic. This means that the reaction absorbs heat from the surroundings. In endothermic reactions, increasing the temperature will cause the reaction to shift towards the products, favoring their formation.
Le Chatelier's principle states that if a change is made to a system at equilibrium, the system will adjust to counteract the change and restore equilibrium. In this case, increasing the temperature will cause the reaction to shift in the direction that absorbs the added heat, which is the side of the products.
Therefore, the correct answer isOption C: increase in temperature, as it will favor the formation of the products of the reaction at equilibrium.