question_answer 12)

Find out the value of equilibrium constant for the following reaction at 298 K: \[2N{{H}_{3}}(g)+C{{O}_{2}}(g)\rightleftharpoons N{{H}_{2}}CON{{H}_{2}}(aq)+{{H}_{2}}O(l)\] Standard Gibbs free energy change\[\Delta {{G}^{{}^\circ }}\]at the given temperature is\[-13.6kJ\,mo{{l}^{-1}}\] .

Answer:

\[\Delta {{G}^{{}^\circ }}=-2.303RT\,{{\log }_{10}}{{K}_{p}}\] \[\log {{K}_{p}}=\frac{-\Delta {{G}^{{}^\circ }}}{2.303RT}\] \[=-\frac{(-13.6\times {{10}^{3}})}{2.303\times 8.314\times 298}\] \[=2.38\] \[{{K}_{p}}=Anti\log (2.38)=2.4\times {{10}^{2}}\]