What is the relationship between ΔG, ΔH, and ΔS at constant temperature?
Practice Questions
1 question
Q1
What is the relationship between ΔG, ΔH, and ΔS at constant temperature?
ΔG = ΔH + TΔS
ΔG = ΔH - TΔS
ΔG = TΔS - ΔH
ΔG = ΔH/ΔS
The relationship is given by the equation ΔG = ΔH - TΔS, where T is the temperature in Kelvin.
Questions & Step-by-step Solutions
1 item
Q
Q: What is the relationship between ΔG, ΔH, and ΔS at constant temperature?
Solution: The relationship is given by the equation ΔG = ΔH - TΔS, where T is the temperature in Kelvin.
Steps: 5
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.
