Calculate the standard Gibbs free energy chan | vedclass

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Question

(A) The relationship between standard Gibbs free energy change $\Delta G^o$ and the equilibrium constant $K_p$ is given by the equation: $\Delta G^o =

Vedclass · Accepted Answer

$162.74 \ kJ \ mol^{-1}$

Vedclass · Answer

(A) The relationship between standard Gibbs free energy change $\Delta G^o$ and the equilibrium constant $K_p$ is given by the equation: $\Delta G^o = -RT \ln K_p$.Given values are $R = 8.314 \ J \ K^{-1} \ mol^{-1}$,$T = 298 \ K$,and $K_p = 3 	imes 10^{-29}$.Substituting these values into the equation:$\Delta G^o = -(8.314 \ J \ K^{-1} \ mol^{-1}) 	imes (298 \ K) 	imes \ln(3 	imes 10^{-29})$.$\Delta G^o = -2477.572 	imes (\ln 3 + \ln 10^{-29})$.$\Delta G^o = -2477.572 	imes (1.0986 - 66.779)$.$\Delta G^o = -2477.572 	imes (-65.6804) \approx 162735 \ J \ mol^{-1}$.Converting to $kJ \ mol^{-1}$,we get $\Delta G^o \approx 162.74 \ kJ \ mol^{-1}$.

Calculate the standard Gibbs free energy change $\Delta G^o$ at $298 \ K$ for the conversion of oxygen to ozone,given by the reaction: $\frac{3}{2} O_{2(g)} \rightleftharpoons O_{3(g)}$. The equilibrium constant $K_p$ for this conversion is $3 \times 10^{-29}$.

Similar Questions

For the following reaction at $50^\circ$ $C$ and at $2 \text{ atm}$ pressure, $2N_2O_5(g) \rightleftharpoons 2N_2O_4(g) + O_2(g)$. $N_2O_5$ is $50\%$ dissociated. The magnitude of standard free energy change at this temperature is $x$. $x = . . . . . . \text{ J mol}^{-1}$.

For an equilibrium reaction,if $\Delta G^{\circ} = 0$,the equilibrium constant $K$ is equal to:

The correct relationship between standard free energy change $(\Delta G^o)$ and equilibrium constant $(K)$ is:

At $320 \ K,$ a gas $A_2$ is $20 \%$ dissociated to $A_{(g)}.$ The standard free energy change at $320 \ K$ and $1 \ atm$ in $J \ mol^{-1}$ is approximately $(R = 8.314 \ J \ K^{-1} \ mol^{-1}; \ \ln \ 2 = 0.693; \ \ln \ 3 = 1.098).$

Identify the relation between the standard Gibbs free energy change $\Delta G^{\circ}$ and the equilibrium constant $K_c$ for a chemical reaction.

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