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For a water gas reaction, C((s)) + H(2)O...

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.

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`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`
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