For the reaction A + B $\rightarrow$ C + D, $\Delta$H° = +40 kJ and $\Delta$S° = +50 J/K. Therefore, the reaction under standard conditions is

Question

Quizplus · Accepted Answer

The positive value of ∆H° indicates that the reaction is endothermic, meaning it requires an input of energy to proceed. The positive value of ∆S° indicates that the reaction becomes more disordered or has an increased entropy, which favors spontaneity. Using the Gibbs free energy equation, ∆G° = ∆H° - T∆S°, we can determine that the reaction will only be spontaneous at temperatures where ∆G° is negative. Since ∆H° is positive and dominates the equation, the reaction is only spontaneous at high temperatures where the negative T∆S° term can counterbalance the positive ∆H° term. Therefore, choice (B) is the correct answer.

For the Reaction a + B →\rightarrow→ C + D Δ\DeltaΔ H° = +40 KJ And

For the Reaction a + B $\rightarrow$ C + D $\Delta$ H° = +40 KJ And