For the reaction K_c = 66.9 at 350ºC and Kc = 50.0 at 448ºC. The reaction has

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For the reaction $H_{2}(g) + I_{2}(g) \rightleftharpoons 2HI(g)$
K_c = 66.9 at 350ºC and Kc = 50.0 at 448ºC. The reaction has

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H_{2}(g) + I_{2}(g) \rightleftharpoons 2HI(g)

log\frac{K_{2}}{K_{1}} = \frac{\Delta H}{2.303R}\left\lbrack \frac{1}{T_{1}} - \frac{1}{T_{2}} \right\rbrack

log\frac{50}{66.9} = \frac{\Delta H}{2.303R}\left\lbrack \frac{1}{623} - \frac{1}{721} \right\rbrack

After calculation negative value of

\Delta

H is obtained.

Source: Grass-G / CH-24 Chemistry Paper 31 Dec..docx

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