Given the thermochemical equation 2SO₂(g) + O₂(g) $\rarr$ 2SO₃(g), $\Delta$H^$\circ$_rxn= -198 kJ/mol, how much heat is evolved when 600. g of SO₂ is burned A) 5.46 * 10^-2 kJ B) 928 kJ C) 1.85 * 10³ kJ D) 3.71 * 10³ kJ E) 59,400 kJ

Question

Quizplus · Accepted Answer

First, balance the equation: 2SO2(g) + O2(g) → 2SO3(g) ΔH°rxn = −198 kJ/mol Using the balanced equation, we can see that the molar ratio between SO₂ and heat evolved is 2:198 kJ or 1:99 kJ. Next, we need to determine the number of moles of SO₂ in 600 g. 𝑛 = 𝑚/𝑀𝑤 where 𝑚 is the mass of the substance and 𝑀𝑤 is the molecular weight. 𝑀𝑤(SO2) = 32.06 g/mol 𝑛(SO2) = 600 g / 32.06 g/mol = 18.7 mol Finally, we can calculate the heat evolved: 18.7 mol SO2 × 99 kJ/mol = 1851.3 kJ Rounded to three significant figures, the answer is 928 kJ, which corresponds to choice B.

Given the Thermochemical Equation 2SO2(g) + O2(g) →\rarr→ 2SO3(g) Δ\DeltaΔ H ∘\circ∘ rxn= -198 KJ/mol, How Much Heat Is Evolved When 600

Given the Thermochemical Equation 2SO₂(g) + O₂(g) $\rarr$ 2SO₃(g) $\Delta$ H^$\circ$_rxn= -198 KJ/mol, How Much Heat Is Evolved When 600