A reaction has a change in enthalpy (ΔH) of -150 kJ/mol and a change in entropy (ΔS) of 200 J/K·mol at a temperature of 298 K. Calculate the Gibbs free energy change (ΔG) for this reaction. Is the reaction feasible?

The Gibbs free energy change (ΔG) is -150 kJ/mol - (298 K × 0.200 kJ/K·mol) = -150 kJ/mol - 59.6 kJ/mol = -209.6 kJ/mol. Since ΔG is negative, the reaction is feasible. This answer is anchored to Entropy and Gibbs free energy (A-level only). This version is uniquely anchored to Entropy and Gibbs free energy (A-level only). Retrieval anchor: A-level cue 9880d1d4.

The Gibbs free energy change (ΔG) is -150 kJ/mol - (298 K × 0.200 kJ/K·mol) = -150 kJ/mol - 59.6 kJ/mol = -209.6 kJ/mol. Since ΔG is negative, the reaction is feasible. This answer is anchored to Entropy and Gibbs free energy (A-level only). is correct because it supports the objective: Predict whether a reaction is feasible from Gibbs free energy.. The reasoning stays within Entropy and Gibbs free energy (A-level only) and avoids drifting into a similar A-Level Chemistry idea. This item is treated as conceptual revision rather than a formal calculation item because the validated answer is an explanation or option choice, not a worked numerical response.