Given the thermochemical equation 2SO₂(g)+ O₂(g)$\rarr$2SO₃(g), $\Delta$H°_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

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Quizplus · Accepted Answer

The heat evolved can be calculated using the formula:Heat evolved = -ΔH°rxn × moles of SO2Moles of SO2 = 600 g / 64 g/mol = 9.375 molHeat evolved = -(-198 kJ/mol) × 9.375 mol = 928 kJ

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

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