The following reaction is performed at 298 , | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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

Vedclass · Accepted Answer

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

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

In a $20 \ L$ vessel,if $1 \ mol$ each of $CO$,$H_2O$,and $CO_2$ are initially present,then for the equilibrium $CO + H_2O \rightleftharpoons CO_2 + H_2$,which of the following is true?

If $8 \, \text{mol}$ of $PCl_5$ is heated in a closed vessel of $10 \, L$ capacity and $25\%$ of it dissociates into $PCl_3$ and $Cl_2$ at equilibrium,then the value of $K_p$ is .....

At $67\,^{\circ}C$ and $1\ bar$ pressure,dinitrogen tetraoxide is $50\%$ dissociated into nitrogen dioxide. $\Delta G^{\circ}$ for the process $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$ is $(R = \frac{25}{3} \ J \ K^{-1} \ mol^{-1}, \ln 2 = 0.7, \ln 3 = 1.1)$.

For the following reactions,equilibrium constants are given:
$S_{(s)} + O_{2(g)} \rightleftharpoons SO_{2(g)}; K_1 = 10^{52}$
$2S_{(s)} + 3O_{2(g)} \rightleftharpoons 2SO_{3(g)}; K_2 = 10^{129}$
The equilibrium constant for the reaction $2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$ is:

Vedclass Test Series

Exam Paper Generator

Online Exam Module

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 $298 \, K$? $(K_p = 1.6 \times 10^{12})$