Which of the following is not correct?

### Core Logic According to the second law of thermodynamics, at constant temperature and pressure, the change in Gibbs free energy (Delta G$\Delta G$) dictates the spontaneity of a process. - If Delta G lt 0$\Delta G \lt 0$ (negative), the process is spontaneous. - If Delta G gt 0$\Delta G \gt 0$ (positive), the process is non-spontaneous. - If Delta G = 0$\Delta G = 0$, the system is in equilibrium (reversible process). Therefore, the statement "Delta G$\Delta G$ is positive for a spontaneous reaction" is factually incorrect. ### Evaluation Rubric / Model Answer null ### Chapter Mix Class 11 Chemistry: Thermodynamics