The standard Gibbs energy change for the reaction
`2SO_2(g) +O_2(g) to 2SO_3` (g)
is `-142 kJ mol^(-1)` at `300` K. Calculate equilibrium constant.

Explanation

To calculate the equilibrium constant (K) for the reaction \( 2SO_2(g) + O_2(g) \rightarrow 2SO_3(g) \) given that the standard Gibbs energy change (\( \Delta G^\circ \)) is \(-142 \, \text{kJ mol}^{-1}\) at \(300 \, \text{K}\), we can use the relationship between Gibbs energy and the equilibrium constant:

\[ \Delta G^\circ = -RT \ln K \]

Where:
- \( R \) is the universal gas constant, \( R = 8.314 \, \text{J mol}^{-1} \text{K}^{-1} \)
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