The correct thermodnamic conditions for the spontaneous reaction at all temperature is:

Options

A. `DeltaH gt 0 and DeltaS lt 0`
B. `DeltaH lt 0 and DeltaS gt 0`
C. `DeltaH lt 0 and DeltaS lt 0`
D. `DeltaH lt 0 and DeltaS = 0`

Answer

B, D

Explanation

We have the Gibbs Helmholtz reaction for spontaneity as
`DeltaG=DeltaH-TDeltaS`
For reaction to be spontaneous , `DeltaG` must be negative . For this , `DeltaH` should be negative and `DeltaS` should be positive.
`therefore DeltaH lt 0 and DeltaS gt 0`
and also `DeltaS=0` shows `DeltaG` a negative quantity.