According to the integrated form of the Van 't Hoff equation, . Which of the following conclusions c — Chemical Equilibrium Chemistry Question

💡 Solution & Explanation

For an endothermic reaction, the RHS is positive, so $\log(K_2/K_1) > 0 \Rightarrow K_2 > K_1$. For an exothermic reaction, the RHS is negative, so $K_2 < K_1$. If $\Delta H^\circ = 0$, the RHS is $0$, so $K_2 = K_1$. Option D is false because exothermic reactions shift backward (become less forward dominant) as T increases.