Describe the differences between the positive and negative free energy of a chemical reaction.

The positive and negative free energy of a chemical reaction differ in their energy requirements.

Chemical reactions involve a transfer of energy, and this energy is measured in terms of free energy. Free energy is the amount of energy available to do work, and it is represented by the symbol ΔG. A negative ΔG indicates that the reaction releases energy, while a positive ΔG indicates that the reaction requires energy.

A reaction with a negative ΔG is exergonic, meaning that it releases energy. This energy can be harnessed to do work, such as powering cellular processes. Exergonic reactions are spontaneous and tend to occur without the need for external energy input. Examples of exergonic reactions include the breakdown of glucose during cellular respiration.

In contrast, a reaction with a positive ΔG is endergonic, meaning that it requires energy input. This energy input can come from a variety of sources, such as sunlight or ATP hydrolysis. Endergonic reactions are non-spontaneous and require external energy input to occur. Examples of endergonic reactions include the synthesis of glucose during photosynthesis.

In summary, the positive and negative free energy of a chemical reaction differ in their energy requirements. A negative ΔG indicates an exergonic reaction that releases energy, while a positive ΔG indicates an endergonic reaction that requires energy input.