Thermodynamics C Question 9
Question 9 - 2024 (31 Jan Shift 1)
Consider the following reaction at $298 \mathrm{~K}$.
$\frac{3}{2} \mathrm{O}{2(\mathrm{~g})} \rightleftharpoons \mathrm{O}{3(\mathrm{~g})} \cdot \mathrm{K}_{\mathrm{P}}=2.47 \times 10^{-29}$.
$\Delta_{\mathrm{r}} \mathrm{G}^{\oplus}$ for the reaction is $\mathrm{kJ}$. (Given $\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1}$ )
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Answer (163)
Solution
$\frac{3}{2} \mathrm{O}{2(\mathrm{~g})} \rightleftharpoons \mathrm{O}{3(\mathrm{~g})} \cdot \mathrm{K}_{\mathrm{p}}=2.47 \times 10^{-29}$.
$\Delta_{\mathrm{r}} \mathrm{G}^{\oplus}=-\mathrm{RT} \ln \mathrm{K}_{\mathrm{P}}$
$=-8.314 \times 10^{-3} \times 298 \times \ln \left(2.47 \times 10^{-29}\right)$
$=-8.314 \times 10^{-3} \times 298 \times(-65.87)$
$=163.19 \mathrm{~kJ}$
