Final Answer:
The Gibbs free energy change with temperature for the reaction can be predicted using the equation ΔG = ΔH - TΔS. Given the values of entropy (ΔS = -189.2 J/mol) and enthalpy (ΔH = -201 kJ/mol), the Gibbs free energy change will decrease with increasing temperature.
Step-by-step explanation:
The Gibbs free energy change (ΔG) is a key parameter that indicates the spontaneity of a chemical reaction. The relationship between Gibbs free energy, enthalpy (ΔH), entropy (ΔS), and temperature (T) is described by the equation ΔG = ΔH - TΔS. In this equation, a negative ΔG suggests a spontaneous reaction.
Given the values ΔS = -189.2 J/mol and ΔH = -201 kJ/mol, it's important to ensure that the units are consistent. Converting ΔH to J/mol (-201 kJ/mol = -201,000 J/mol), the equation becomes ΔG = -201,000 J/mol - T(-189.2 J/mol). As temperature increases, the impact of the temperature-dependent term (-TΔS) becomes more significant. Since ΔS is negative, the overall effect is a decrease in ΔG with increasing temperature.
In practical terms, this means that the reaction becomes more spontaneous at higher temperatures. The negative ΔG indicates that the reaction is thermodynamically favorable, and as the temperature rises, the system tends to favor this spontaneous process even more. Understanding the temperature dependence of Gibbs free energy provides insights into the conditions under which a reaction is energetically favorable.