Final answer:
To calculate the absolute value of the difference in Gibbs free energy (ΔG) between alternative chair conformations, use the formula ΔG° = ΔH° - TΔS°, resulting in a nonspontaneous process at room temperature with a ΔG° of 58.45 kJ/mol.
Step-by-step explanation:
The student's question involves calculating the absolute value of the difference in the Gibbs free energy (ΔG) between alternative chair conformations of a compound. Using the provided equations and data, the Gibbs free energy change (ΔG°) can be calculated for the reaction process at standard conditions, particularly at 25 °C (298.15 K). The formula to calculate this is: ΔG° = ΔH° - TΔS°, where ΔH° is the change in enthalpy, T is the absolute temperature in Kelvin, and ΔS° is the change in entropy. Both methods provided in the reference material, the one using the calculated enthalpy and entropy change and the other involving using tabulated values, result in the calculation of ΔG° as 58.45 kJ/mol, which indicates that the process is nonspontaneous at room temperature since the value is positive.