91Ó°ÊÓ

Enthalpy change, denoted as \( \Delta H \), represents the total energy change in a system during a chemical reaction. It's measured in kilojoules (kJ) per mole or sometimes given in joules (J) depending on the context.
In any chemical process, energy is either absorbed or released:

• If \( \Delta H \) is negative, the reaction is exothermic, releasing energy to the surroundings.
• If \( \Delta H \) is positive, the reaction is endothermic, absorbing energy from the surroundings.

For example, in our original exercise, the \( \Delta H \) value is \(-20.5 \mathrm{kJ}\), indicating that the system releases energy and is exothermic.
Such a release of energy tends to favor spontaneous reactions, but other factors, like entropy and temperature, also play a significant role in determining spontaneity.

Entropy, symbolized as \( \Delta S \), is a measure of disorder or randomness in a system. Generally expressed in joules per Kelvin (J/K) or kilojoules per Kelvin (kJ/K), it provides insight into the distribution of energy within a system.
When evaluating reactions:

• If \( \Delta S \) is positive, the disorder in the system increases, potentially favoring spontaneity.
• If \( \Delta S \) is negative, the system becomes less disordered, which can sometimes oppose spontaneity.

In the given exercise, the \( \Delta S \) value is \(-35.0 \mathrm{J/K}\), which converts to \(-0.035 \mathrm{kJ/K}\). The negative entropy change suggests a decrease in disorder, which may counteract some of the effects of an exothermic reaction.
However, both changes in entropy and enthalpy must be considered with temperature to fully determine a process's spontaneity.

Spontaneity in chemical reactions depends on the Gibbs Free Energy change, \( \Delta G \). A key formula for determining spontaneity is:\[ \Delta G = \Delta H - T \Delta S \]Where:

• \(\Delta G\) is the Gibbs Free Energy change.
• \(\Delta H\) is the change in enthalpy.
• \(T\) is the temperature in Kelvin.
• \(\Delta S\) is the change in entropy.

If \( \Delta G \) is negative, the reaction is spontaneous, meaning it can occur without outside intervention. Meanwhile, a positive \( \Delta G \) indicates a nonspontaneous reaction, which requires energy input.
In the exercise above, substituting the values into the formula gives:\[ \Delta G = (-20.5 \text{ kJ}) - (298 \text{ K}) \times (-0.035 \text{ kJ/K}) = -10.07 \text{ kJ} \]A result of \(-10.07 \text{ kJ}\) reveals a spontaneous process at the specified temperature.
This example illustrates how enthalpy, entropy, and temperature collectively influence whether a chemical reaction proceeds on its own.