Enthalpy can be expressed in both Joules per mole and Calories per mole.

The unit of entropy is Joules per mole per Kelvin (J/mol·K).

The work done by a gas during an isothermal expansion is W = nRT ln(Vf/Vi).

The work done by an ideal gas during an isothermal expansion is W = nRT ln(Vf/Vi).

The nature of the solvent does not directly affect the Gibbs Free Energy of a reaction; it is primarily influenced by temperature, pressure, and concentration.

While temperature, pressure, and concentration of reactants affect Gibbs Free Energy, the nature of the solvent does not directly affect ΔG.

The first law of thermodynamics states that energy cannot be created or destroyed, only transformed.

Hess's Law states that the total enthalpy change for a reaction is the same, regardless of the number of steps in the reaction.

Hess's Law states that the total enthalpy change for a reaction is the same, regardless of the number of steps taken.

The Second Law of Thermodynamics states that the total entropy of an isolated system can never decrease over time.

A reaction is favored when it has low ΔH (exothermic) and high ΔS (increased disorder).

Increasing temperature for an exothermic reaction (ΔH < 0) can lead to a decrease in Gibbs Free Energy, making the reaction more spontaneous.

A high temperature and high ΔS will favor a negative ΔG, making the process spontaneous.

A positive ΔG can occur at low temperatures when the enthalpy is high, making the reaction non-spontaneous.

A spontaneous reaction occurs when ΔG < 0. This is true for ΔH < 0 and ΔS > 0, as it leads to a negative ΔG.

The correct relation is ΔG = ΔH - TΔS.

The correct relation is ΔG = ΔH - TΔS.

The nature of the solvent does not directly affect Gibbs Free Energy; it is primarily influenced by temperature, pressure, and concentration.

The enthalpy change of a reaction is independent of the pathway taken, as it is a state function.

While temperature, volume, and the nature of the substance affect entropy, pressure does not directly affect the entropy of a system in a significant way.

While temperature, pressure, and concentration of reactants affect Gibbs Free Energy, the nature of the solvent does not directly affect ΔG.

CO2(g) has a higher enthalpy of formation compared to the elements in their standard states.

Steam has the highest entropy at 25°C because it is in the gaseous state, which has more disorder compared to solid (ice) and liquid (water).

Water vapor has the highest entropy because gases have greater disorder compared to liquids and solids.

Water vapor has the highest entropy due to its gaseous state, which has more disorder compared to solids and liquids.

Water vapor at 100 °C has the highest entropy due to its gaseous state, which has more disorder compared to the liquid and solid states.

H2O(l) has a higher standard molar entropy than the diatomic gases due to its molecular complexity and interactions.

The correct expression for Gibbs Free Energy is ΔG = ΔH - TΔS.

Gibbs Free Energy can be expressed in various units, including Joules per mole, kilojoules, and calories.

Enthalpy is a state function, while work and heat are not state functions as they depend on the path taken.