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

Find out the value of equilibrium constant for the following reaction

1.	Find out the value of equilibrium constant for the following reaction at 298 K. 2NH_(3(g)) + CO_(2(g)) hArr NH_(2) CONH_(2(aq) ) + H_(2) O_((l)) Standard Gibbs energy change, Delta_(r) G^( Theta ) at the given temperature is -13.6 "kJ mol"^(-1).
Answer» Solution :We know, `LOG K= (- Delta_(r) G^( Theta ) )/( 2.303 "RT" ) ` `= ((13.6 xx 10^(3) "J MOL"^(-1) ) )/( 2.303 (8.314 "JK"^(-1)"mol"^(-1) ) (298) )=2.38` Hence, `K=` antilog `2.38 = 2.4 xx 10^(2)`