ΔG = 0 occurs at equilibrium, where the forward and reverse reactions occur at the same rate.

ΔG equals ΔH when the entropy change (ΔS) is zero, indicating no change in disorder.

ΔG is zero at equilibrium, indicating no net change in the concentrations of reactants and products.

The enthalpy change for a reaction can be calculated using bond energies, standard enthalpies of formation, and calorimetry.

A positive enthalpy change indicates that the reaction absorbs heat, thus it is endothermic.

The enthalpy of vaporization is the heat required to convert a liquid into a gas at constant temperature and pressure.

The enthalpy of vaporization of water is approximately 40.79 kJ/mol.

The enthalpy of vaporization of water is approximately 2260 kJ/mol.

For a phase transition at constant temperature, the change in entropy is given by ΔS = ΔH/T, where ΔH is the enthalpy change.

The change in entropy for a reaction is calculated using the formula ΔS = ΣS(products) - ΣS(reactants).

According to the third law of thermodynamics, the entropy of a perfect crystal at absolute zero is zero.

According to the third law of thermodynamics, the entropy of a perfect crystal at absolute zero is zero, which is the minimum value.

The third law of thermodynamics states that the entropy of a perfect crystal approaches zero as the temperature approaches absolute zero.

According to the third law of thermodynamics, the entropy of a perfect crystal at absolute zero is exactly zero.

The third law of thermodynamics states that the entropy of a perfect crystalline substance approaches zero as the temperature approaches absolute zero.

According to the third law of thermodynamics, the entropy of a perfect crystalline substance at absolute zero is zero.

A large negative value of ΔG indicates that the reaction is highly spontaneous and favors the formation of products.

A negative ΔG indicates that the reaction is spontaneous under the given conditions.

A positive ΔG indicates that the reaction is non-spontaneous.

A positive ΔG indicates that the reaction is non-spontaneous.

A positive ΔS indicates an increase in disorder or randomness in the system.

A ΔG value of zero indicates that the reaction is at equilibrium, meaning the forward and reverse reactions occur at the same rate.

The Gibbs free energy change indicates the spontaneity of a reaction; a negative value suggests spontaneity.

The enthalpy of reaction refers to the heat absorbed or released at constant pressure.

Entropy is a measure of the disorder or randomness in a system.

Gibbs free energy indicates the maximum reversible work that can be performed by a thermodynamic system at constant temperature and pressure.

For an endothermic reaction, increasing temperature generally decreases ΔG, making the reaction more favorable.

The entropy of a system increases when it undergoes an irreversible process.

In an endothermic reaction, heat is absorbed from the surroundings, resulting in a positive change in enthalpy.

In an exothermic reaction, heat is released, resulting in a negative change in enthalpy.