Question

Find out the value of equilibrium constant for the following reaction at 298 K, \[\ce{2NH3_{(g)} + CO2_{(g)} ⇌ NH2 - COONH2_{(aq)} + H2O_{(l)}}\] Gibbs Standard energy change 298 K = –13.6 kJ mol⁻¹.

Answer 1

Given: Δ⁰G = -13.6 kJ mol^-1

R = 8.314 JK^-1 mol^-1, T = 298 K.

 \[\ce{2NH3_{(g)} + CO2_{(g)} ⇌ NH2 - COONH2_{(aq)} + H2O_{(l)}}\]

Δ⁰G = `-2.303nRTlogK`

`log K = (-13.6xx10^3)/(2.303xx8.314xx298)`

`logK=2.38`

`K="Antilog"(2.38)`

`= 239.9 ≈ 240`

`K = 2.40xx10^2`