For a reaction at constant temperature and pressure, which of the following is t

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Question: For a reaction at constant temperature and pressure, which of the following is true?

Options:

Correct Answer: ΔG = ΔH - TΔS

Solution:

The correct relationship at constant temperature and pressure is ΔG = ΔH - TΔS.

For a reaction at constant temperature and pressure, which of the following is true?

For a reaction at constant temperature and pressure, which of the following is true?

Correct Answer: ΔG = ΔH - TΔS

Step 1: Understand that ΔG represents the change in Gibbs free energy of a system.
Step 2: Recognize that ΔH represents the change in enthalpy (total heat content) of the system.
Step 3: Identify that ΔS represents the change in entropy (disorder) of the system.
Step 4: Note that T is the absolute temperature in Kelvin.
Step 5: Remember that at constant temperature and pressure, the relationship between these quantities is given by the equation ΔG = ΔH - TΔS.
Step 6: Conclude that this equation helps determine if a reaction is spontaneous (ΔG < 0) or not (ΔG > 0).

Gibbs Free Energy – The relationship between Gibbs free energy (ΔG), enthalpy (ΔH), and entropy (ΔS) at constant temperature (T) and pressure.
Thermodynamic Relationships – Understanding how changes in enthalpy and entropy affect the spontaneity of a reaction.