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Find out the value of equilibrium consta...

Find out the value of equilibrium constant for the following reaction at 298 K.
`2NH_(3)(g)+CO_(2)(g)hArrNH_(2)CONH_(2)(aq)+H_(2)O(1)`
Standard Gibbs energy change, `Delta_(r)G^(Ө)` at the given temperature is `-13.6 kJ "mol"^(-1)`

Text Solution

Verified by Experts

`log K = -(DeltaG^(@))/(2.303RT)`
`DeltaG^(@) = -13.6 kJ mol^(-1), R = 8.314 JK^(-1)mol^(-1)`,
`T = 298 K`
`log K = -(-13.6 xx 10^(3))/(2.303 xx 8.314 xx 298)`
`log K = 2.38`
`therefore K = 2.40 xx 10^(2)`.
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