If `Delta H gt 0` and `Delta S gt 0`, the reaction proceeds spontaneously when :-

For a non-spontaneous reaction, at 30^(@)C, DeltaH gt 0 & DeltaS gt 0 . The reaction becomes spontaneous, by

At a given temperature and pressure, for a chemical reaction DeltaH gt0 and DeltaS lt 0 . The reaction is non-spontaneous at all temperature. But the reverse reaction is spontaneous at all temperature-give reason.

DeltaH gt DeltaE for the reaction

A particular reaction at 27^(@)C for which DeltaH gt 0 and DeltaS gt 0 is found to be non-spontaneous. The reaction may proceed spontaneously if

A particular reaction at 27^(@)C for which DeltaH gt 0 and DeltaS gt 0 is found to be non-spontaneous. The reaction may proceed spontaneously if

A change in the free energy of a system at constant temperature and pressure will be: Delta_(sys)G = Delta_(sys)H -T Delta_(sys)S At constant temperature and pressure Delta_(sys) G lt 0 (spontaneous) Delta_(sys)G = 0 (equilibrium) Delta_(sys)G gt 0 (non-spontaneous) If both DeltaH and Deltas are negative, the reaction will be spontaneous