For the reaction,2 NH_{3(g)} + CO_{2(g)} righ | vedclass

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Question

(A) The relationship between standard Gibbs energy change and equilibrium constant is given by: $\Delta G^{\circ} = -RT \ln K$ or $\Delta G^{\circ} =

Vedclass · Accepted Answer

$2.88 	imes 10^2$

Vedclass · Answer

(A) The relationship between standard Gibbs energy change and equilibrium constant is given by: $\Delta G^{\circ} = -RT \ln K$ or $\Delta G^{\circ} = -2.303 RT \log K$. Given: $\Delta G^{\circ} = 13.9 \ kJ \ mol^{-1} = 13900 \ J \ mol^{-1}$,$R = 8.314 \ J \ K^{-1} \ mol^{-1}$,$T = 295 \ K$. Substituting the values: $13900 = -2.303 	imes 8.314 	imes 295 	imes \log K$. $\log K = \frac{-13900}{2.303 	imes 8.314 	imes 295} = \frac{-13900}{5650.3} \approx -2.46$. Wait,the standard Gibbs energy change for the formation of urea from ammonia and carbon dioxide is typically negative. Assuming the value provided is $\Delta G^{\circ} = -13.9 \ kJ \ mol^{-1}$: $\log K = \frac{13900}{5650.3} \approx 2.46$. $K = 10^{2.46} \approx 288.4 = 2.88 	imes 10^2$. Hence,option $(A)$ is correct.

For the reaction,$2 NH_{3(g)} + CO_{2(g)} \rightleftharpoons NH_2CONH_{2(aq)} + H_2O_{(l)}$,find the value of the equilibrium constant at $295 \ K$. Given,the standard Gibbs energy change at the given temperature is $13.9 \ kJ \ mol^{-1}$.

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