For independent process at 300K . Process / kJmol ^ - 1 / JK ^ - 1...

The relation between change in Gibbs free energy, change in enthalpy and change in entropy can be written as follows,

$\Delta G = \Delta H - T \Delta S$

If $∆ G$ is $+ ve$ , then the process is said to be non-spontaneous and if $∆ G$ is $- ve$ then the process is said to be spontaneous.

$A: \Delta G\left({Jmol}^{- 1}\right) = - 25 \times {10}^{3} + 80 \times 300: - ve$

$B: \Delta G\left({Jmol}^{- 1}\right) = - 22 \times {10}^{3} - 40 \times 300: - ve$

$C: \Delta G\left({Jmol}^{- 1}\right) = 25 \times {10}^{3} + 300 \times 50; + ve$

$D: \Delta G\left({Jmol}^{- 1}\right) = 22 \times {10}^{3} - 20 \times 300: + ve$

Processes $C$ and $D$ are non-spontaneous.