Hydrolysis of sucrose gives
`"Sucrose" +H_(2)OhArr"Glucose + Fructose"`
Equilibrium constant `K_(c)` for the reaction is `2xx10^(13)` at `300 K`. Calculate `DeltaG^(ɵ)` at `300 K`.

Explanation

To calculate the standard Gibbs free energy change (ΔG°) for the hydrolysis of sucrose at 300 K, we can use the relationship between ΔG° and the equilibrium constant (Kc). The formula is:

\[ \Delta G^\circ = -2.303 \, R \, T \, \log K_c \]

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