Question: In which of the following scenarios is ΔG equal to ΔH?
Options:
At high temperatures with ΔS = 0.
At low temperatures with ΔS = 0.
At constant pressure and temperature.
In a phase transition.
Correct Answer: In a phase transition.
Solution:
During a phase transition, such as melting or boiling, ΔG equals ΔH because the system is at equilibrium.
In which of the following scenarios is ΔG equal to ΔH?
Practice Questions
Q1
In which of the following scenarios is ΔG equal to ΔH?
At high temperatures with ΔS = 0.
At low temperatures with ΔS = 0.
At constant pressure and temperature.
In a phase transition.
Questions & Step-by-Step Solutions
In which of the following scenarios is ΔG equal to ΔH?
Step 1: Understand what ΔG and ΔH represent. ΔG is the change in Gibbs free energy, and ΔH is the change in enthalpy (heat content).
Step 2: Know that ΔG indicates whether a process is spontaneous (can happen on its own) or not.
Step 3: Recognize that during a phase transition (like melting ice to water or boiling water to steam), the system is at equilibrium.
Step 4: At equilibrium, the energy changes in the system balance out, which means ΔG equals ΔH.
Step 5: Conclude that ΔG equals ΔH specifically during phase transitions because the system is not gaining or losing energy in a way that drives it away from equilibrium.
Gibbs Free Energy (ΔG) – ΔG represents the change in free energy of a system, indicating the spontaneity of a process.
Enthalpy (ΔH) – ΔH represents the change in enthalpy, or heat content, of a system during a process.
Phase Transition – A phase transition is a process where a substance changes from one state of matter to another, such as solid to liquid or liquid to gas.
Equilibrium – A state where the forward and reverse processes occur at the same rate, resulting in no net change in the system.
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