Consider the following chemical reaction:CaSO₄(s) + 2H₂O (g) $\rarr$ CaSO₄ - 2H₂O (s)This reaction is exothermic.

Question

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Given that the reaction is exothermic, it implies that it releases energy to the surroundings, which tends to favor spontaneity. However, without information on the entropy change (ΔS) and the exact enthalpy change (ΔH), we cannot definitively say it is spontaneous at all temperatures. Generally, exothermic reactions (negative ΔH) are more likely to be spontaneous at lower temperatures because the temperature dependence of the Gibbs free energy equation (ΔG = ΔH - TΔS) means that at lower temperatures, the TΔS term has less impact, making ΔG more likely to be negative (indicative of spontaneity).

Consider the Following Chemical Reaction:CaSO4(s) + 2H2O (G) →\rarr→ CaSO4 - 2H2O (S)This Reaction Is Exothermic

Consider the Following Chemical Reaction:CaSO₄(s) + 2H₂O (G) $\rarr$ CaSO₄ - 2H₂O (S)This Reaction Is Exothermic