Question

Find out the value of equilibrium constant for the following reaction at 298 K.

2NH₃ (g) + CO₂ (g) ⇋ NH₂CONH₂ (aq) + H₂O(I)

Standard Gibbs energy change, ∆_rG^Θ at the given temperature is −13.6 kJ mol^-1 .

Answer 1

Given, T = 298 K

∆_rG^Θ = −13.6 kJ mol⁻¹

R = 8.314 J K⁻¹ mol^-1

K = ?

∴ ∆_rG^Θ K = −2.303RT log K

or log K = \(\frac{-\Delta_rG^\ominus}{2.303\,RT}\)

= \(\frac{-(-13.6 \times10^3Jmol^{-1})}{2.303\times8.314\,JK^{-1}\times298\,K}\)

= 2.38

\(\therefore\) K = antilog 2.38

= 2.4 × 10²