How does entropy effect enthalpy?

Entropy and enthalpy are two distinct effects that don't interact.

Both terms refer to energy: entropy indicates a substance's degree of disorder or degrees of freedom, whereas enthalpy indicates a substance's stability as a result of its bonding.

The determination of the feasibility of a reaction is dependent on both entropy and enthalpy, which are combined to form the quantity known as free energy. The free energy change is calculated as the enthalpy change minus the entropy change times the absolute temperature. If the free energy change is negative, the reaction is considered feasible.

Entropy and enthalpy are both thermodynamic properties, but they affect each other differently. Entropy measures the disorder or randomness of a system, while enthalpy measures the heat content of a system.

Changes in entropy can affect changes in enthalpy through the equation:

ΔG = ΔH - TΔS

where ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy.

Entropy affects enthalpy through the temperature term in the equation. As entropy increases (ΔS > 0), the temperature term (TΔS) becomes larger, potentially leading to a decrease in the overall change in enthalpy (ΔH). Conversely, if entropy decreases (ΔS < 0), the temperature term (TΔS) becomes smaller, potentially leading to an increase in the overall change in enthalpy (ΔH).

In summary, changes in entropy can influence changes in enthalpy through their interplay in the Gibbs free energy equation.