A reaction will never the spontaneous at any temperature and pressure if

Options

A. `DeltaS =+ve, DeltaH =+ve`
B. `DeltaS =+ve, DeltaH =- ve`
C. `DeltaS =- ve, DeltaH =+ve`
D. `DeltaS =-ve, DeltaH =- ve`

Explanation

To determine when a reaction will never be spontaneous at any temperature and pressure, we need to analyze the Gibbs free energy change (ΔG) for the reaction. The spontaneity of a reaction is determined by the sign of ΔG, which is given by the equation:

\[ \Delta G = \Delta H - T \Delta S \]

Where:
- ΔG = Gibbs free energy change
- ΔH = Change in enthalpy
- T = Temperature in Kelvin
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