Chemistry · EQUILIBRIUM

For the hydrolysis of sucrose at \( 300\text{ K} \), the equilibrium constant is \( K = 2.0 \times 10^{13} \). What is the standard Gibbs energy change \( \Delta G^\circ \) for this reaction? (Given: \( R = 8.314\text{ J mol}^{-1}\text{K}^{-1} \), \( \ln(2.0 \times 10^{13}) = 30.627 \))

1. \( +7.64 \times 10^4\text{ J mol}^{-1} \)
2. \( -3.82 \times 10^4\text{ J mol}^{-1} \)
3. \( -7.64 \times 10^4\text{ J mol}^{-1} \)
4. \( +3.82 \times 10^4\text{ J mol}^{-1} \)