At $298 \ K$,$\Delta_r G^{\ominus}$ for the following reaction is $165.469 \ kJ \ mol^{-1}$. What is the equilibrium constant for this reaction? $(R = 8.3 \ J \ mol^{-1} \ K^{-1})$
$\frac{3}{2} O_{2(g)} \longrightarrow O_{3(g)}$
$\frac{3}{2} O_{2(g)} \longrightarrow O_{3(g)}$
- A$10^{29}$
- B$10^{-29}$
- C$5 \times 10^{-27}$
- D$5 \times 10^{+27}$
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