For the reaction, 2SO 2 (g) + O 2 (g) → 2SO 3 (g); ΔH = -44.0 kcal at 300 K. If 4.0 moles of SO 2 reacts with 2.0 moles of O 2 at constant pressure of 1.0 atm and temperature 300 K to form SO 3 , then

Question

For the reaction, 2SO 2 (g) + O 2 (g) → 2SO 3 (g); ΔH = -44.0 kcal at 300 K. If 4.0 moles of SO 2 reacts with 2.0 moles of O 2 at constant pressure of 1.0 atm and temperature 300 K to form SO 3 , then the correct statement(s) is/are (one or more than one correct)

TestHub · Accepted Answer

4 mol SO 2 and 2 mol O 2 are exactly twice the equation, so ΔH = 2(-44.0) = -88 kcal, and heat released at constant pressure is 88 kcal (b true). Gas moles go from 6 to 4, Δn g = -2. Work magnitude = 2 × 2 × 300 = 1200 cal = 1.2 kcal (done on the system), so (a) with 2.4 kcal is false. ΔU = ΔH - Δn g RT = -88 - (-2)(0.6) = -88 + 1.2 = -86.8 kcal, so internal energy decreases by 86.8 kcal (c true, d false). Ans (b),(c).

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