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(B) The standard free energy change for the reaction is given by $\Delta G^{\circ} = -RT \ln K_p$.For the reaction $2 NO_{(g)} + O_{2(g)} \rightleftha

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$0.5 [2 	imes 86600 - R(298) \ln (1.6 	imes 10^{12})]$

Vedclass · Answer

(B) The standard free energy change for the reaction is given by $\Delta G^{\circ} = -RT \ln K_p$.For the reaction $2 NO_{(g)} + O_{2(g)} ightleftharpoons 2 NO_{2(g)}$,the standard free energy change is $\Delta G^{\circ} = 2 \Delta G^{\circ}_{f}(NO_2) - [2 \Delta G^{\circ}_{f}(NO) + \Delta G^{\circ}_{f}(O_2)]$.Since $\Delta G^{\circ}_{f}(O_2) = 0$,we have $\Delta G^{\circ} = 2 \Delta G^{\circ}_{f}(NO_2) - 2 \Delta G^{\circ}_{f}(NO)$.Given $\Delta G^{\circ}_{f}(NO) = 86.6 \, kJ/mol = 86600 \, J/mol$ and $T = 298 \, K$,we substitute these into the equation:$-R(298) \ln (1.6 	imes 10^{12}) = 2 \Delta G^{\circ}_{f}(NO_2) - 2(86600)$.Rearranging for $\Delta G^{\circ}_{f}(NO_2)$:$2 \Delta G^{\circ}_{f}(NO_2) = 2(86600) - R(298) \ln (1.6 	imes 10^{12})$.$\Delta G^{\circ}_{f}(NO_2) = 0.5 [2 	imes 86600 - R(298) \ln (1.6 	imes 10^{12})]$.

The following reaction is performed at $298 \, K$.
$2 NO_{(g)} + O_{2(g)} \rightleftharpoons 2 NO_{2(g)}$
The standard free energy of formation of $NO_{(g)}$ is $86.6 \, kJ/mol$ at $298 \, K$. What is the standard free energy of formation of $NO_{2(g)}$ at $298 \, K$? $(K_p = 1.6 \times 10^{12})$

Similar Questions

Consider the following two equilibrium reactions:
$i$. $2NH_{3(g)} \rightleftharpoons N_{2(g)} + 3H_{2(g)}$
$ii$. $2ND_{3(g)} \rightleftharpoons N_{2(g)} + 3D_{2(g)}$
What is the difference in their equilibrium constants $(K_c)$?

Consider the following liquid-vapour equilibrium.
$Liquid \rightleftharpoons Vapour$
Which of the following relations is correct?

If the pressure in a reaction vessel for the following reaction is increased by decreasing the volume,what will happen to the concentrations of $CO$ and $CO_2$ ?
$H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)} + \text{Heat}$

$A$ mixture of $SO_2$ and $O_2$ at $5 \, atm$ pressure reacts $30\%$ until equilibrium is reached. Determine the total pressure of the equilibrium mixture in $atm$.
$2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$

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The following reaction is performed at $298 \, K$.$2 NO_{(g)} + O_{2(g)} \rightleftharpoons 2 NO_{2(g)}$The standard free energy of formation of $NO_{(g)}$ is $86.6 \, kJ/mol$ at $298 \, K$. What is the standard free energy of formation of $NO_{2(g)}$ at $298 \, K$? $(K_p = 1.6 \times 10^{12})$

Similar Questions

Consider the following two equilibrium reactions:$i$. $2NH_{3(g)} \rightleftharpoons N_{2(g)} + 3H_{2(g)}$$ii$. $2ND_{3(g)} \rightleftharpoons N_{2(g)} + 3D_{2(g)}$What is the difference in their equilibrium constants $(K_c)$?

Consider the following liquid-vapour equilibrium.$Liquid \rightleftharpoons Vapour$Which of the following relations is correct?

If the pressure in a reaction vessel for the following reaction is increased by decreasing the volume,what will happen to the concentrations of $CO$ and $CO_2$ ?$H_2O_{(g)} + CO_{(g)} \rightleftharpoons H_{2(g)} + CO_{2(g)} + \text{Heat}$

$A$ mixture of $SO_2$ and $O_2$ at $5 \, atm$ pressure reacts $30\%$ until equilibrium is reached. Determine the total pressure of the equilibrium mixture in $atm$.$2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$