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

₹0.0

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

Options:

Correct Answer: ΔG = ΔH - TΔS

Solution:

The relationship is given by the equation ΔG = ΔH - TΔS, where T is the temperature in Kelvin.

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.

No concepts available.