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Enthalpy change is a measure of the total heat content in a system under constant pressure. It is symbolized as \( \Delta H \) and is typically expressed in units of joules per mole. In a reaction, enthalpy change indicates whether heat is absorbed or released. Enthalpy changes may be either positive or negative:

• A positive \( \Delta H \) means the reaction absorbs heat (endothermic).
• A negative \( \Delta H \) signifies that the reaction releases heat (exothermic).

In our exercise, the given \( \Delta H \) is \( 30 \, \text{kJ} \, \text{mol}^{-1} \), which is a positive value. This tells us that the reaction \( \mathrm{Br}_{2}(\ell)+\mathrm{Cl}_{2}(\mathrm{~g}) \longrightarrow 2 \mathrm{BrCl}(\mathrm{g}) \)requires the input of heat from its surroundings to proceed. Understanding enthalpy change is crucial because it directly affects the Gibbs free energy and helps predict the feasibility of reactions.

Entropy, represented by \( \Delta S \), refers to the degree of disorder or randomness in a system. Entropy change measures the change in this disorder as a result of a chemical reaction. It is measured in joules per Kelvin per mole.A positive \( \Delta S \) indicates an increase in disorder, while a negative \( \Delta S \) suggests a decrease. In our specific reaction, \( \Delta S \) is \( 105 \, \text{J} \, \text{K}^{-1} \, \text{mol}^{-1} \), a positive number. This means that the products (gaseous \( \mathrm{BrCl} \)) are more disordered than the reactants (liquid \( \mathrm{Br}_{2} \) and gaseous \( \mathrm{Cl}_{2} \)).The change in entropy plays a vital role in determining the spontaneity of a process. A reaction with a significant increase in entropy can proceed spontaneously even if it absorbs heat (endothermic), as seen in processes like the melting of ice.

Chemical equilibrium occurs when a reaction's forward and backward rates are equal, resulting in no net change in the concentration of reactants and products over time. At equilibrium, the Gibbs free energy change, \( \Delta G \), is zero.In the context of the Gibbs equation, \( \Delta G = \Delta H - T \Delta S \), equilibrium is reached when the enthalpy change of the system balances out the product of the temperature and the entropy change. Thus, no further reaction occurs as the system's energy is minimized.Understanding the concept of equilibrium is key to predicting and controlling chemical processes. It not only determines the extent of reactions but also influences conditions such as pressure and concentration that favor either forward or reverse reactions.

Calculating the temperature at which a chemical reaction reaches equilibrium involves using the Gibbs free energy equation rearranged as \( T = \frac{\Delta H}{\Delta S} \). To find this temperature, use the given values of enthalpy and entropy change.In the problem, the enthalpy change \( \Delta H \) is first converted from kilojoules to joules \((30,000 \, \text{J} \, \text{mol}^{-1})\).Then, dividing \( \Delta H \) by \( \Delta S \), \[ T = \frac{30,000 \, \text{J} \, \text{mol}^{-1}}{105 \, \text{J} \, \text{K}^{-1} \, \text{mol}^{-1}} \approx 285.71 \, \text{K} \]This calculation shows the specific temperature at which the system will reach equilibrium. At this point, the effect of the enthalpy and entropy changes are balanced, and there is no net energy change, making it a critical parameter for understanding reaction conditions.