Answer:
The difference in energy (G) between the products & reactants favours a reaction toward the molecule with lower energy to reach equilibrium.
Step-by-step explanation:
In a chemical reaction, the Gibbs free energy (G) represents the thermodynamic potential that dictates whether the reaction will proceed. The difference in energy (ΔG) between the products and reactants determines the direction of the reaction. If ΔG is negative, the reaction is exergonic, favoring the formation of products. Conversely, if ΔG is positive, the reaction is endergonic, requiring an input of energy.
To reach equilibrium, the system tends to minimize its free energy, favoring the formation of the molecule with lower energy. This is because a lower energy state is more stable and thermodynamically favorable.
Understanding the energetics of chemical reactions and equilibrium is fundamental in fields like chemistry and biochemistry, providing insights into reaction spontaneity and the stability of molecular systems.