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  • For the reaction, A(g) + B(g) → C(g) + D(g), H0  and S0 are, respectively, −29.8 kJ mol−1 and −0.100 kJ K−1 mol&mi

For the reaction, A(g) + B(g) → C(g) + D(g), H0  and S0 are, respectively, −29.8 kJ mol−1 and −0.100 kJ K−1 mol−1 at 298 K.  The equilibrium constant for the reaction at 298 K is :

Option: 1

1.0 × 10−10


Option: 2

 1.0 × 1010


Option: 3

10


Option: 4

 1


Answers (1)

\\\Delta G^{\circ}=\Delta H^{\circ}-T . \Delta S^{\circ} \\ =-29.8+298\times(0.1) \\ =-29.8+29.8 \\ \because \Delta G^{\circ}=0 \\ \\ \text{apply relation between } \\ $\Delta G^{\circ}=-R T \ln K_{e q}$ \\ $\therefore K_{e q}=1$

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Kshitij

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