Consider the following gas phase reaction:H_ 2 (g) + Cl_ 2 (g) 2H… - Vidyadip

Question

Consider the following gas phase reaction:$\text{H}_{2}\text{(g)} + \text{Cl}_{2} \text{(g)} \rightleftharpoons\text{2HCl(g)}$
$\Delta\text{H}^{\circ} = -92\text{kJ}, \ \Delta\text{S}^{\circ} = -95\text{JK}^{-1}$
Calculate the equilibrium constant, $K_p$ at 298 K for this reaction.

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Answer

$\Delta \text{G}^{\circ} =\Delta \text{H}^{\circ} - \text{T}\Delta\text{S}^{\circ}$$ = 92\text{kJ} \frac{298 \times 95}{1000}\text{kJ} = -64\text{kJ}$
$\Delta \text{G}^{\circ} = -2.303 \text{RT} \log \text{k}_{\text{p}}$
$-64\text{kJ} = \frac{-2.303 \times 8.314\times 298\text{K} }{1000}\log \text{K}_{\text{p}}$
$\log \text{K}_{\text{sp}} = \frac{-64\text{kJ}}{-5.7058\text{kJ}} = 11.2166$
$\text{K}_{\text{p}} = \text{Antilog } 11.2166$

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