The following reaction is performed at $298\;K$ $2NO(g) +O_2(g) \to 2NO_2(g)$ . 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 $298\;K\; (K_p = 1.6 \times 10^{12})$

Question

$\begin{array}{1 1} 86600+Rs(298)ln(1.6 \times 10^{12}) \\ 8600 - \frac{ln(1.6 \times 10^{12})}{R(298)}\\ 0.5 [2 \times 86,600 -R(298) ln(1.6 \times 10^{12})] \\ R(298) ln(1.6 \times 10^{12} )- 86600 \end{array} $