Find out the value of equilibrium constant for the following reaction at 298K, 2NH_(3(g)) +CO_(2(g)) hArr NH_2CONH_(2(aq))+H_2O_((l)) Standard Gibbs energy change, DeltaG_r^0 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 298K, 2NH_(3(g)) +CO_(2(g)) hArr NH_2CONH_(2(aq))+H_2O_((l)) Standard Gibbs energy change, DeltaG_r^0 at the given temperature is "-13.6 kJ mol"^(-1) .
Answer» Solution :Given : T=298 K `DeltaG_r^0=-13.6 "kJ mol"^(-1)` `=-13600 "J mol"^(-1)` `DeltaG^0=-2.303 RT log K_(eq)` `log K_(eq)=(-DeltaG^0)/(2.303RT)` `log K_(eq)=("13.6 kJ mol"^(-1))/(2.303xx8.314xx10^(-3) JK^(-1) mol^(-1)xx298K)` `logK_(eq)=2.38` `K_(eq)`=antilog(2.38) `K_(eq)`=239.88