For a spontaneous process, the change in Gibbs free energy (ΔG) is related to en

For a spontaneous process, the change in Gibbs free energy (ΔG) is related to entropy (ΔS) how?

For a spontaneous process, the change in Gibbs free energy (ΔG) is related to entropy (ΔS) how?

Step 1: Understand that Gibbs free energy (ΔG) is a measure of the energy available to do work in a system.
Step 2: Know that for a process to be spontaneous, it must occur without needing to be driven by an external force.
Step 3: Recognize that the change in Gibbs free energy (ΔG) is calculated using the formula ΔG = ΔH - TΔS.
Step 4: Identify that ΔH represents the change in enthalpy (total heat content) of the system.
Step 5: Understand that T is the absolute temperature in Kelvin.
Step 6: Realize that ΔS is the change in entropy, which measures the disorder or randomness in the system.
Step 7: Remember that for a process to be spontaneous, ΔG must be negative (ΔG < 0).
Step 8: Conclude that if ΔS is positive (increased disorder), it can help make ΔG negative, promoting spontaneity.

Gibbs Free Energy – Gibbs free energy (ΔG) is a thermodynamic potential that measures the maximum reversible work obtainable from a system at constant temperature and pressure.
Entropy – Entropy (ΔS) is a measure of the disorder or randomness in a system, and it plays a crucial role in determining the spontaneity of a process.
Spontaneous Processes – A spontaneous process is one that occurs without needing to be driven by an external force, typically characterized by a negative change in Gibbs free energy (ΔG < 0).
Thermodynamic Equation – The equation ΔG = ΔH - TΔS relates the change in Gibbs free energy to the change in enthalpy (ΔH) and the change in entropy (ΔS) at a given temperature (T).