Chemistry - Thermodynamics - II Question with Solution | TestHub

For the reaction :
$\text{2}\text{NO(g)}\text{+}{\text{O}}_{\text{2}}\text{(g)}\to \text{2}{\text{NO}}_{\text{2}}\text{(g)}$
$\text{ΔG}\text{=}\left\{{\text{2Δ}}_{\text{f}}\text{G}\left({\text{NO}}_{\text{2}}\right)\right\}-\left\{{\text{2Δ}}_{\text{f}}\text{G}\left(\text{NO}\right)\text{+}{\text{Δ}}_{\text{f}}\text{G}\left({\text{O}}_{\text{2}}\right)\right\}$
$=\left(2\times 51\text{.}84\right)-\left(2\times 86\text{.}69+0\right)$
$=103\text{.}68-173\text{.}38$
$=-69\text{.}7\text{kJ/mol}$
$\because \text{ΔG}$is negative
so, the reaction is spontaneous