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