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?

Question

Quizplus · Accepted Answer

First, calculate the moles of SO₂ burned: 600 g SO₂ x (1 mol SO₂/272 g SO₂) = 2.21 mol SO₂ Next, use the thermochemical equation to calculate the heat evolved: 2 mol SO₂ x (-198 kJ/mol) = -396 kJ The negative sign indicates the reaction is exothermic, and we need to change the sign to give a positive value for the heat evolved. -(-396 kJ) = 396 kJ, which is equivalent to 9.28 x 10^2 kJ (in scientific notation). The best choice is therefore B, which gives the answer with the correct units and numerical value.

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