Endergonic reaction

Another way to phrase this is that useful energy must be absorbed from the surroundings into the workable system for the reaction to happen.

A positive value of ΔG° therefore implies so that starting from molar stoichiometric quantities such a reaction would move backwards toward equilibrium, not forwards.

Examples of endergonic reactions in cells include protein synthesis, and the Na+/K+ pump which drives nerve conduction and muscle contraction.

All physical and chemical systems in the universe follow the second law of thermodynamics and proceed in a downhill, i.e., exergonic, direction.

equals the change in the Gibbs free energy after completion of a chemical reaction.

Endergonic reactions can be achieved if they are either pulled or pushed by an exergonic (stability increasing, negative change in free energy) process.

However, the reaction can proceed because having reached the transition state, it rapidly evolves via an exergonic process to the more stable final products.

An endergonic reaction (such as photosynthesis ) is a reaction that requires energy to be driven. Endergonic means "absorbing energy in the form of work." The activation energy for the reaction is typically larger than the overall energy of the exergonic reaction (1). Endergonic reactions are nonspontaneous. The progress of the reaction is shown by the line. The change of Gibbs free energy ( Δ G ) during an endergonic reaction is a positive value because energy is gained (2).