The equilibrium constant of a reaction is `1xx10^(20)` at `300 K`. The standard free energy change for this reaction is :

Options

A. `-115kJ`
B. `+115 kJ`
C. `+166 kJ`
D. `-166 kJ`

Explanation

To find the standard free energy change (\( \Delta G^\circ \)) for the reaction given the equilibrium constant (\( K \)), we can use the following formula:

\[ \Delta G^\circ = -2.303 \cdot R \cdot T \cdot \log(K) \]

Where:
- \( R \) is the universal gas constant, approximately \( 8.314 \, \text{J/mol·K} \)
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