For a spontaneous reaction, both ΔG (Gibbs Free Energy) and ΔE (Change in Internal Energy) are negative.
ΔG represents the maximum amount of work that can be obtained from a reaction at constant temperature and pressure. For a spontaneous reaction, the Gibbs free energy change, ΔG, is negative, indicating that the reaction will proceed spontaneously in that direction.
ΔE is the change in the amount of internal energy of a system during a reaction. A negative value of ΔE indicates that the energy released by the reaction is greater than the energy required to start the reaction, which means that the reaction is spontaneous.
Therefore, for a spontaneous reaction both ΔG and ΔE will be negative.
What are the values of ΔG and ΔE for a spontaneous reaction
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