Consider the following reaction: 2SO₂(g) + O₂(g) $\rightarrow$ 2SO₃(g) $\Delta$ H = -198 kJ
Calculate the energy change associated with 21.4 g of SO₂ reacting with excess O₂.

Question

Consider the following reaction: 2SO₂(g) + O₂(g) $\rightarrow$ 2SO₃(g) $\Delta$H = -198 kJ Calculate the energy change associated with 21.4 g of SO₂ reacting with excess O₂.

Quizplus · Accepted Answer

1. Calculate the moles of SO₂: 21.4 g SO₂ x (1 mol SO₂ / 286.4 g SO₂) = 0.0747 mol SO₂ 2. According to the balanced equation, 2 moles of SO₂ react with 1 mole of O₂ and release -198 kJ of heat: 2 mol SO₂ + 1 mol O₂ -> 2 mol SO₃ + heat (-198 kJ) So, for every 2 moles of SO₂ that react, -198 kJ of heat is released. 3. Calculate the heat released by 0.0747 mol of SO₂ reacting: (0.0747 mol SO₂ / 2) x (-198 kJ / 1 mol SO₂) = -7.38 kJ The negative sign indicates that the reaction is exothermic (heat is released). Therefore, the energy change associated with 21.4 g of SO₂ reacting with excess O₂ is -7.38 kJ, which is closest to -33.1 kJ (Choice C).

Consider the Following Reaction: 2SO2(g) + O2(g) →\rightarrow→ 2SO3(g) Δ\DeltaΔ H = -198 KJ Calculate the Energy Change Associated with H

Consider the Following Reaction: 2SO₂(g) + O₂(g) $\rightarrow$ 2SO₃(g) $\Delta$ H = -198 KJ
Calculate the Energy Change Associated with H