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)`

Explanation

To find the equilibrium constant \( K \) for the reaction

\[ 2NH_3(g) + CO_2(g) \rightleftharpoons NH_2CONH_2(aq) + H_2O(l) \]

at 298 K, given the standard Gibbs energy change \( \Delta_r G^\circ = -13.6 \, \text{kJ mol}^{-1} \), we can use the relationship between Gibbs free energy and the equilibrium constant:

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