Which of the following reactions has the smallest value of $\Delta$S $\circ$ ? A) NH₃(g) + HCl(g) $\rarr$NH₄Cl(s) B) 2H₂(l) + O₂(l) $\rarr$ 2H₂O(g) C) N₂(g) + 3H₂(g) $\rarr$ 2NH₃(g) D) K(s) + O₂(g) $\rarr$ KO₂(s) E) BaCl₂.2H₂O(s) $\rarr$ BaCl₂(s) + 2H₂O(g)

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Quizplus · Accepted Answer

The reaction with the smallest value of ΔG° (Gibbs free energy change) is typically one that involves the formation of a solid from gases, as this process is highly exergonic (releases energy). Among the given options, reaction A involves the formation of a solid compound (NH4Cl) from gaseous reactants (NH3 and HCl), which is likely to have a very negative ΔG°, indicating a highly spontaneous reaction under standard conditions.

Which of the Following Reactions Has the Smallest Value Of \Delta