Imagine a hypothetical reacion for which,
�H = 0 kJ · mol−1. Considering the Le
Chatelier principle, which of the following
statements is true?
a. Raising the temperature of the system will have no effect.
b. Raising the temperature of the system will cause the reaction to shift left.
c. Raising the temperature of the system will cause the reaction to shift right.
To determine the effect of temperature on a reaction, we need to consider the principle of Le Chatelier. According to Le Chatelier's principle, if a system at equilibrium is subjected to a change, the system will respond in a direction that minimizes the change.
In this case, the reaction has a ΔH value of 0 kJ/mol, which means it is not exothermic or endothermic. A reaction with a ΔH of 0 indicates that the forward and reverse reactions have the same energy change. For such a reaction, the effect of temperature is different compared to reactions with non-zero ΔH values.
When the temperature of a reaction with ΔH = 0 kJ/mol is increased, it means that the system is being supplied with thermal energy. The reaction will respond to minimize this change in temperature. Since the system is already at equilibrium, the reaction does not have a specific direction to shift towards to reach equilibrium.
Therefore, option a is correct: Raising the temperature of the system will have no effect on the equilibrium position. The reaction will remain at equilibrium, and the concentrations of the reactants and products will stay the same.