Correct Answer - Option 3 : ΔG < 0 and ΔS > 0
Concept:
Spontaneous Processes
- Spontaneous processes are those that can proceed without any outside intervention.
- Entropy, temperature and heat flow all play a major role in spontaneity.
- A thermodynamic quantity, the Gibbs free energy (G) combines these factors to predict the spontaneity of a process
\(\Delta G\, = \,\Delta H\, - \,T\Delta S\)
If a process releases heat ( \(\Delta H\,\) is negative ) and has increased in entropy ( \(\Delta S\) positive ), it will always be spontaneous.
The value of \(\Delta G\) for spontaneous process is negative.
Explanation:
Summary of conditions for spontaneity
- \(\Delta G\) < 0 , \(\Delta S\) > 0
The reaction is spontaneous in the forward direction.
- \(\Delta G\) > 0 , \(\Delta S\) < 0
The reaction is non-spontaneous in the forward direction.
- \(\Delta G\) = 0 , \(\Delta S\) = 0
The system is at equilibrium.
Appropriate condition for the Spontaneity of a process is ΔG < 0 and ΔS > 0
