Each of the following statements is false. Rewrite each so that it makes a correct statement about free energy.
a. ΔGuniverse > 0 for any spontaneous process.
b. ΔH = ΔG TΔS.
a. ΔGuniverse < 0 for any spontaneous process.
Explanation: The correct statement is that the change in Gibbs free energy (ΔG) for any spontaneous process is negative, indicating that the process occurs spontaneously.
b. ΔH = ΔG + TΔS.
Explanation: The correct statement is the Gibbs-Helmholtz equation, which relates the change in enthalpy (ΔH) to the change in Gibbs free energy (ΔG) and the change in entropy (ΔS) at a given temperature (T).
a. To make a correct statement about free energy, we need to understand the relationship between ΔG (change in free energy), ΔH (change in enthalpy), T (temperature), and ΔS (change in entropy).
The correct statement is: "ΔGuniverse < 0 for any spontaneous process."
Explanation: Free energy (ΔG) is a measure of the energy available to do useful work in a system. For any spontaneous process, the change in free energy of the universe (ΔGuniverse) must be negative. This means that the system is undergoing a reaction that occurs naturally, without requiring an input of energy.
b. The given statement already correctly describes the relationship between ΔH, ΔG, T, and ΔS.
Explanation: The equation ΔH = ΔG + TΔS is known as the Gibbs-Helmholtz equation. It represents the relationship between the change in enthalpy (ΔH), the change in free energy (ΔG), the temperature (T), and the change in entropy (ΔS). This equation allows us to link the thermodynamic properties of a system and determine the spontaneity of a reaction based on the sign of ΔG.