Question: Which of the following statements is true regarding Gibbs Free Energy?
Options:
ΔG is always positive for spontaneous processes.
ΔG = ΔH - TΔS.
ΔG can never be negative.
ΔG is independent of temperature.
Correct Answer: ΔG = ΔH - TΔS.
Solution:
The correct equation for Gibbs Free Energy is ΔG = ΔH - TΔS, which relates enthalpy, entropy, and temperature.
Which of the following statements is true regarding Gibbs Free Energy?
Practice Questions
Q1
Which of the following statements is true regarding Gibbs Free Energy?
ΔG is always positive for spontaneous processes.
ΔG = ΔH - TΔS.
ΔG can never be negative.
ΔG is independent of temperature.
Questions & Step-by-Step Solutions
Which of the following statements is true regarding Gibbs Free Energy?
Correct Answer: ΔG = ΔH - TΔS
Step 1: Understand what Gibbs Free Energy (ΔG) is. It helps predict if a reaction will happen spontaneously.
Step 2: Learn the components of the Gibbs Free Energy equation: ΔG = ΔH - TΔS.
Step 3: Identify what each symbol means: ΔH is the change in enthalpy (heat content), T is the temperature in Kelvin, and ΔS is the change in entropy (disorder).
Step 4: Recognize that a negative ΔG means the reaction is spontaneous, while a positive ΔG means it is not.
Step 5: Remember that the equation shows how enthalpy and entropy affect the spontaneity of a reaction.
No concepts available.
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