Respuesta :
65.3% yield of H2SO4 if 100g of So2 is completely consumed producing 100 g of H2SO4.
we have to calculate the theoretical yield to calculate percentage yield. It is used go compare the yield of the product with what could have obtained with theory, if all the reactant converted into no loss. the expression for percentage yield is ,
%yield= (Actual yield / theoretical yield) . 100
Theoretical yield is calculated base don the stoichiometry of the chemical reaction and Actual yield is experimentally determined.
The balanced chemical reaction for this is,
2SO₂ + O₂ + 2H₂O → 2H₂SO₄
Molar mass is the mass of the sample of the compound divided by the amount of the substance .
Molar mass of SO₂ = 32 + (16 × 2) = 64 g/mole
Mass of SO₂ = 2 × 64 = 128 g
Molar mass of H₂SO₄ = (1 × 2) + 32 + (16 × 4) = 98 g/mole
Mass of H₂SO₄ = 2 × 98 = 196 g
128 g of SO₂ reacted to produce 196 g of H₂SO₄ .
100 g of SO₂ will react to produce = (100 × 196) / 128 = 153.125 g of H₂SO₄
Finally, we have to determine the percentage yield of H₂SO₄. We have the value of Actual yield of H₂SO₄ = 100 g . Theoretical yield of H₂SO₄ = 153.125 g .
Percentage yield = (Actual /Theoretical) × 100
Percentage yield of H₂SO₄ = (100 / 153.125) × 100
= 65.3%
So the percentage yield of H2SO4 is 65.3%
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