Test: Relationship between Equilibrium Constant K & Gibbs Free Energy (July 22) - NEET MCQ

The relationship between ΔG and the equilibrium constant (K) for a reaction is given by the equation ΔG = ΔG° + RT ln K. This equation relates the free energy change (ΔG) to the standard free energy change (ΔG°) and the equilibrium constant (K).

In a reversible reaction, ?G is negative in both the forward and backward reactions. This indicates that the free energy of the reaction mixture is lower than the free energy of both the reactants and products.

The equation for calculating the change in Gibbs free energy (ΔG) when there is no phase change in the reaction is ΔG = ΔH - TΔS, as mentioned in the provided text. This equation considers the enthalpy (ΔH) and entropy (ΔS) of the system.

A negative value of ΔG° indicates that the reaction is spontaneous with K >> 1. This means that the products are favored at equilibrium, and the reaction proceeds in the forward direction. The negative value of ΔG° indicates that the reaction releases energy.

The relationship between Gibbs free energy (ΔG) and the electromotive force (EMF) of a cell in a galvanic cell is given by the equation ΔG = nFE(cell), where n is the number of moles of electrons involved, F is the Faraday constant, and E(cell) is the EMF of the cell. This equation relates the free energy change to the electrical work done by the cell.

The unit of standard Gibbs free energy of formation (?fG°) is Joules per mole (J/mol). It represents the change in Gibbs free energy when one mole of a substance is formed from its component elements in their standard states.

According to Gibbs free energy, a reaction is considered spontaneous when ΔG is less than 0. This indicates that the reaction can occur spontaneously and release energy. When ΔG is greater than 0, the reaction is non-spontaneous.

The equation for Gibbs free energy (G) is given by G = H - TS, as stated in the provided text. This equation represents the maximum amount of work that can be extracted from a closed system at constant temperature and pressure. It accounts for the enthalpy (H), temperature (T), and entropy (S) of the system.