For a hypothetical reaction, the standard enthalpy change ( H ) and standard entropy change ( S ) are -40 kJ mol ⁻¹ and -100 J K ⁻¹ mol ⁻¹ respectively. Under which of the following temperature conditions will the reaction be spontaneous?

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Correct answer: D. T < 400 K

For a reaction to be spontaneous, the change in Gibbs free energy ( G ) must be negative. G = H - T S Given: H = -40 kJ mol ⁻¹ = -40000 J mol ⁻¹ S = -100 J K ⁻¹ mol ⁻¹ Substituting the values into the inequality: -40000 - T(-100) -40000 + 100T 100T T Thus, the reaction will be spontaneous at temperatures less than 400 K . Answer: T < 400 K

For a hypothetical reaction, the standard enthalpy change ( H ) and standard entropy change ( S ) are -40 kJ mol ⁻¹ and -100 J K ⁻¹ mol ⁻¹ respectively. Under which of the following temperature conditions will the reaction be spontaneous?

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