For a water gas reaction, C_((s)) + H_(2)O_((g)) hArr CO_((g)) + H_(2(g)) at 1000 K, the standard Gibb's energy change is -8.1 kJ mol^(-1). Calculate the value of equilibrium constant.

For a water gas reaction, C_((s)) + H_(2)O_((g)) hArr CO_((g)) + H_(2(

1.	For a water gas reaction, C_((s)) + H_(2)O_((g)) hArr CO_((g)) + H_(2(g)) at 1000 K, the standard Gibb's energy change is -8.1 kJ mol^(-1). Calculate the value of equilibrium constant.
Answer» SOLUTION :`Delta G^(@) = -2.303 RT log K` `log K = (-Delta G^(@))/(2.303 xx RT)` `= (-(-8.1 xx 10^(3)J))/2.303 xx 8.314 xx 1273 = 0.3323` , TAKING antilogs of both sides. `:. K = "ANTILOG" (0.3323) = 2.14 g`