Question

For a given exothermic reaction, $K_p$ and $K_p^{\prime }$ are the equilibrium constants at temperatures $T_1$ and $T_2$ respectively. Assuming that heat of reaction is constant in temperatures range between $T_1$ and $T_2$. It is readily observation that :
(Given, $T_2>T_1$)

• A. $K_P>K_P^{\prime }$
• B. $K_P<K_P^{\prime }$
• C. $K_P=K_P^{\prime }$
• D. $K_{=}\frac{1}{K_P^{\prime }}$

Answer 1

The correct option is A $K_P>K_P^{\prime }$

$\log \frac{K_2}{K_1}=\frac{\Delta H^0}{2.303R}(\frac{1}{T_1}-\frac{1}{T_2})$
$T_2>T_1$ so $K_p<K_p^{\prime }$ (exothermic reaction)
(Given, $T_2>T_1$)
$\log \frac{K_2}{K_1}=\frac{\Delta H^0}{2.303R}(\frac{1}{T_1}-\frac{1}{T_2})$