Final answer:
The value of ΔH (kJ/mol) for the reaction can be determined using the equation ΔG° = ΔH° - TΔS°, where ΔG° is the standard free energy change, ΔH° is the standard enthalpy change, ΔS° is the standard entropy change, and T is the temperature in Kelvin. From the given equation of the straight line, y = -10.195x + 171.674, where y represents ΔG (in kJ/mol) and x represents T (in K), we can identify that the slope of the line (-10.195) represents -ΔH°, as ΔH° is the negative of the slope. Therefore, the value of ΔH° for the reaction is 10.195 kJ/mol.
Step-by-step explanation:
The value of ΔH (kJ/mol) for the reaction can be determined using the equation ΔG° = ΔH° - TΔS°, where ΔG° is the standard free energy change, ΔH° is the standard enthalpy change, ΔS° is the standard entropy change, and T is the temperature in Kelvin.
From the given equation of the straight line, y = -10.195x + 171.674, where y represents ΔG (in kJ/mol) and x represents T (in K), we can identify that the slope of the line (-10.195) represents -ΔH°, as ΔH° is the negative of the slope.
Therefore, the value of ΔH° for the reaction is 10.195 kJ/mol.