Question

The following reaction is performed at $298K$
$2NO\left(g\right)+O_2\left(g\right)\rightleftharpoons 2{NO}_2\left(g\right)$
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 ${NO}_2\left(g\right)$ at $298K$?
$(K_P=1.6\times {10}^{12})$

• A. $0.5[2\times 86,600-R(298)\ln (1.6\times {10}^{12})$
• B. $R\left(298\right)\ln (1.6\times {10}^{12})-86,600$
• C. $86,600+R\left(298\right)\ln 1.6\times {10}^{12})$
• D. $86,600-\frac{\ln (1.6\times {10}^{12})}{R(298}$

Answer 1

The correct option is A $0.5[2\times 86,600-R(298)\ln (1.6\times {10}^{12})$