What is the relationship between ΔG, ΔH, and ΔS at constant temperature?

What is the relationship between ΔG, ΔH, and ΔS at constant temperature?

Step 1: Understand the symbols. ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy (heat content), and ΔS is the change in entropy (disorder).
Step 2: Know that T is the temperature measured in Kelvin.
Step 3: Learn the equation that relates these quantities: ΔG = ΔH - TΔS.
Step 4: Recognize that this equation shows how Gibbs free energy (ΔG) depends on both the heat content (ΔH) and the disorder (ΔS) of a system at a constant temperature (T).
Step 5: Remember that if ΔG is negative, the process is spontaneous; if positive, it is non-spontaneous.

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