Consider the reaction 2SO₃(g)$\rightarrow$2SO₂(g)+ O₂(g) Which statement is true for this reaction? A) $\Delta$S 0 C) $\Delta$S = 0 D) S_m^o = 0 for O₂(g)

Question

Consider the reaction 2SO₃(g)$\rightarrow$2SO₂(g)+ O₂(g) Which statement is true for this reaction? A) $\Delta$S < 0 B) $\Delta$S > 0 C) $\Delta$S = 0 D) S_m^o = 0 for O₂(g)

Quizplus · Accepted Answer

According to the reaction, two molecules of SO₃(g) react to form one molecule of F1F1F102SO₂(g) and one molecule of O₂(g). This means that the reaction releases energy and is exothermic, which is reflected in a negative ΔF1F1F1S1 value. Therefore, statement B is correct as ΔF1F1F1S1F1F1F10S must be negative. Statements A and C are incorrect since they suggest a positive or zero value for ΔF1F1F1S1F1F1F10S, which is not true for an exothermic reaction. Statement D is not relevant for determining the directionality of the reaction or its energetic properties.

Consider the Reaction 2SO3(g) →\rightarrow→ 2SO2(g)+ O2(g) Which Statement Is True for This Reaction? A)

Consider the Reaction
2SO₃(g) $\rightarrow$ 2SO₂(g)+ O₂(g)
Which Statement Is True for This Reaction?
A)