For the reaction, A(g) + B(g) $ \to $ C(g) + D(g), $\Delta $Ho and $\Delta $So 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 :

Question

For the reaction,
A(g) + B(g) $ \to $ C(g) + D(g), $\Delta $H^o and $\Delta $S^o 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 :

1.0 $ \times $ 10^$-$10

1.0 $ \times $ 10¹⁰

Solution

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