1. Tardigrade
  2. Question
  3. Chemistry
  4. For the reaction, 2NH3(g)+CO2(g) leftharpoons NH2CONH2(aq)+H2O(l) Standard Gibbs energy change, ΔrG° at the given temperature is -13.6 KJ mol-1 The value of equilibrium constant for the above reaction at 298 K is

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Q. For the reaction,
$2NH_{3(g)}+CO_{2(g)} \rightleftharpoons NH_{2}CONH_{2(aq)}+H_{2}O_{(l)}$
Standard Gibbs energy change, $\Delta_{r}G^{\circ}$ at the given temperature is $-13.6\,KJ\,mol^{-1}$ The value of equilibrium constant for the above reaction at $298\, K$ is

Thermodynamics

Solution:

We know , $log\,K =\frac{-\Delta\,G^{\circ}}{2.303RT}$
$=-\frac{(-13.6 \times 10^{3} J\,mol^{-1})}{2.303(8.314\,JK^{-1}\,mol^{-1})(298\,K)}=2.38$
Hence, $K$ = antilog $2.38=2.4 \times 10^{2}$