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(A) Given: $\Delta H^{\ominus} = 77.2 \ kJ \ mol^{-1} = 77200 \ J \ mol^{-1}$,$T = 400 \ K$,$\Delta S = 122 \ J \ K^{-1} \ mol^{-1}$,$R = 8.314 \ J \

Vedclass · Accepted Answer

$37$

Vedclass · Answer

(A) Given: $\Delta H^{\ominus} = 77.2 \ kJ \ mol^{-1} = 77200 \ J \ mol^{-1}$,$T = 400 \ K$,$\Delta S = 122 \ J \ K^{-1} \ mol^{-1}$,$R = 8.314 \ J \ K^{-1} \ mol^{-1}$.Using the relation $\Delta G^{\ominus} = \Delta H^{\ominus} - T \Delta S$:$\Delta G^{\ominus} = 77200 - (400 	imes 122) = 77200 - 48800 = 28400 \ J \ mol^{-1}$.Using the relation $\Delta G^{\ominus} = -2.303 \ RT \log K$:$28400 = -2.303 	imes 8.314 	imes 400 	imes \log K$.$28400 = -7657.6 	imes \log K$.$\log K = -28400 / 7657.6 \approx -3.708$.Since $\log K = -3.708 = -37.08 	imes 10^{-1}$,the value is approximately $-37$.

Compound	$\Delta_f H^\circ$ $(kJ \ mol^{-1})$	$S^\circ$ $(J \ mol^{-1} \ K^{-1})$
$XY(g)$	$42$	$200$
$X_2(g)$	$8$	$140$
$Y_2(g)$	$80$	$250$

For a certain thermochemical reaction $M \rightarrow N$ at $T = 400 \ K$,$\Delta H^{\ominus} = 77.2 \ kJ \ mol^{-1}$ and $\Delta S = 122 \ J \ K^{-1} \ mol^{-1}$,the value of $\log K$ is $ . . . . . . \times 10^{-1}$.

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