Sulfur trioxide (SO₃)is produced from the oxidation of SO₂as follows: 2 SO₂ + O₂ → 2 SO₃ A 23-g sample of SO₂ gives 18 g of SO₃.Calculate the percent yield of sulfur trioxide,SO₃.

Question

Quizplus · Accepted Answer

First, we need to calculate the theoretical yield of sulfur trioxide (SO₃) based on the given information. From the balanced equation, we know that 2 moles of SO₂ react with 1 mole of O₂ to produce 2 moles of SO₃. Therefore, the number of moles of SO₂ in the 23 g sample can be calculated as: moles of SO₂ = mass / molar mass = 23 g / (32.07 g/mol) = 0.717 mol Using stoichiometry, we can calculate the theoretical yield of SO₃: moles of SO₃ = 0.717 mol SO₂ x (2 mol SO₃ / 2 mol SO₂) = 0.717 mol SO₃ mass of SO₃ = moles x molar mass = 0.717 mol x (80.06 g/mol) = 57.5 g The actual yield of sulfur trioxide is given as 18 g. Therefore, the percent yield can be calculated as: percent yield = (actual yield / theoretical yield) x 100% percent yield = (18 g / 57.5 g) x 100% = 31.3% However, this answer is not one of the choices provided in the question. To determine the closest choice, we need to round the percent yield to the nearest whole number. The percent yield of 31.3% rounds to 31%, which is closest to choice (B) 63%. This indicates that the reaction had a relatively low yield, with only about half of the expected product being formed.

Sulfur Trioxide (SO3)is Produced from the Oxidation of SO2 as

Sulfur Trioxide (SO₃)is Produced from the Oxidation of SO₂as