Find out the value of equilibrium constant for the following reaction at `298K, 2 NH_(3)(g) + CO_(2) (g) hArr NH_(2)CONH_(2) (aq) + H_(2)O (l)` Standard Gibbs energy change, `Delta G_(r)^(0)` at the given temperature is `-13.6" kJ mol"^(-1)`.

Explanation

`T = 298 K`
`Delta G_(r)^(0) =-136.6" kJ mol"^(-1)`
`=-13600" kJ mol"^(-1)`
`Delta G^(0) =-2.303" RT log K"_(eq)`
`log K_(eq) =(-Delta G^(0))/(2.303 RT)`
`log K_(eq) =(13.6" kJ mol"^(-1))/(2.303xx8.314xx10^(-3) JK^(-1)" mol"^(-1) xx298 K)`
`log K_(eq) =2.38`
`K_(eq) =" antilog "(2.38)`
`K_(eq) =239.88`