The dependence of the equilibrium constant on temperature is given by the integrated Van't Hoff equa — Chemical Equilibrium Chemistry Question

💡 Solution & Explanation

If $T_2 > T_1$, the term $(T_2-T_1)/(T_1 T_2)$ is positive. For an endothermic reaction ($\Delta H^\circ > 0$), the right side is positive, making $\log(K_2/K_1) > 0$ and $K_2 > K_1$. For an exothermic reaction ($\Delta H^\circ < 0$), it is negative, so $K_2 < K_1$. If $\Delta H^\circ = 0$, $K_2 = K_1$. Option D is false because the slope is $-\Delta H^\circ / (2.303 R)$ due to the base-10 logarithm.