Question

How is entropy related to the spontaneity of a reaction?

Answer 1

Hint: 1)The second law of thermodynamics says that the entropy of the universe consistently increments for an spontaneous process: \[\Delta {S_{universe}} = \Delta {S_{system}} + \Delta {S_{surrounding}} > 0\]
2)A consistent temperature and pressure, the adjustment in Gibbs free energy is defined as
 \[\Delta G = \Delta H - T\Delta S\]
3)The spontaneity of a process can rely upon the temperature

Complete step by step answer:
Entropy (S) is a proportion of the disorder in a system.
In a closed system, entropy consistently increases after some time. In an open system, energy can be added to a system to cause a lessening in entropy, however this isn't really a spontaneous reaction.
In the event that entropy (disorder) increases, and the reaction enthalpy is exothermic (\[\Delta H < 0\]) or
pitifully endothermic (\[\Delta H > 0\] and small), the reaction is for the most part spontaneous.
The Gibbs free energy condition is:
\[\Delta G = \Delta H - T\Delta S\]
A reaction will be spontaneous if the adjustment in G, \[\Delta G\] , is negative.
For the result of temperature times \[\Delta S\] , where\[\Delta S\] is the change in entropy, if the change in entropy is positive (disorder increases), then \[T\delta S\], when subtracted, gets negative.
Since the cosmos (discernible universe) is basically a closed system, entropy will keep on expanding until the universe basically stops to exist.

Note: When \[\Delta G < 0\] , the process is exergonic and will continue spontaneously the forward direction to form more products.
When \[\Delta G > 0\] , the process is endergonic and not spontaneous in the forward direction. All things being equal, it will continue spontaneously in the opposite direction to make more beginning materials.
When \[\Delta G = 0\] , the system is in equilibrium and the concentrations of the products and reactants will stay consistent.