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Gibbs free energy ($G$) is the measure of the usable energy that can do work at a constant temperature and pressure. In biochemistry, it's used to predict the spontaneity of reactions: a negative $\Delta G$ indicates a spontaneous reaction, which is fundamental in metabolic pathways.

The first law, also known as the law of energy conservation, states that energy cannot be created or destroyed in an isolated system. In biochemistry, this principle underpins the understanding that the energy in biological systems is transformed, such as when ATP is hydrolyzed to ADP and phosphate to release energy.

Activation energy is the energy required to initiate a chemical reaction. Biochemically, this concept is crucial to understanding how enzymes lower the activation energy of reactions to facilitate biological processes.

Entropy ($S$) is a measure of the disorder or randomness in a system. In the context of biochemistry, changes in entropy can drive biomolecular processes and affect protein folding, ligand binding, and the stability of nucleic acids and proteins.

An endergonic reaction is one in which the Gibbs free energy change ($\Delta G$) is positive, and energy is absorbed from the surroundings. Endergonic reactions in biochemical pathways require coupling to exergonic reactions to proceed, like the synthesis of ATP.

An exergonic reaction has a negative Gibbs free energy change ($\Delta G$), and energy is released into the surroundings. These reactions drive biochemical processes, such as the break down of glucose during cellular respiration.

The second law states that the entropy of an isolated system always increases over time. Applied to biochemistry, it explains the directionality of metabolic reactions and the need for organisms to continually obtain energy from their environment to maintain order.