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.

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

Increasing temperature will make ΔG more negative for a reaction with a negative ΔH and positive ΔS, enhancing spontaneity.

For a reaction with ΔH > 0 and ΔS < 0, increasing temperature will make ΔG more positive, thus decreasing spontaneity.

At equilibrium, the Gibbs Free Energy change (ΔG) is zero, indicating that the system is at its lowest energy state.

A negative ΔG (< 0) indicates that a reaction is spontaneous under the given conditions.

The relationship is given by ΔG = -RT ln(K), where R is the gas constant and T is the temperature in Kelvin.

The relationship is given by ΔG = -RT ln K, where R is the gas constant and T is temperature.

The relationship is given by ΔG = -RT ln(K), where R is the gas constant and T is the temperature in Kelvin.

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

Gibbs Free Energy is crucial for predicting the spontaneity and direction of a chemical reaction.

ΔGf° indicates the energy change when a compound is formed from its elements in their standard states.

ΔG° depends on the specific reaction and its conditions.

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.

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.

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

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.