Question

In Haber's process of manufacturing of ammonia,
$N_2\left(g\right)+3H_2\left(g\right)\to 2N{H}_3\left(g\right):H_{{25}^{\circ }C}^0=-92.2kJ$

Molecule	$N_2\left(g\right)$	$H_2\left(g\right)$	$N{H}_3\left(g\right)$
$C_p\left(J{K}^{-1}mol{e}^{-1}\right)$	29.1	28.8	35.1

If $C_p$ is independent of temperature, then, reaction at ${100}^{\circ }C$ as compared to that of ${25}^{\circ }C$ will be:

• A. more endothermic
• B. less endothermic
• C. more exothermic
• D. less exothermic

Answer 1

The correct option is C more exothermic

$\Delta H=C_p\Delta T$. If $C_p$ is independent of the temperature, The value of $\Delta H$ become more negative and the reaction would be more exothermic.