Finding Percent Yield

Question

Consider this reaction, which occurs in the atmosphere and contributes to photochemical smog:

SO₂(g) + H₂O(l) →H₂SO₃(g)

If there is 18.03 g SO₂ and excess H₂O present, the reaction yields 16.5 g H₂SO₃. Calculate the percent yield for the reaction.

Answer 1

SO₂(g) + H₂O(l) →H₂SO₃(g)

If there is 18.03 g SO₂ and excess H₂O present, the reaction yields 16.5 g H₂SO₃. 

18.03 g SO2 x (1 mol SO2/64.07 g SO2) x (1 mol H2SO3/1 mol SO2) x (82.07 g H2SO3/1 mol H2SO3) = 23.10 g H2SO4 the theoretical yield

The actual yield: 16.5 g H₂SO₃

_{%y = AY/TY x 100 = (16.5 g/ 23.1 g) x 100 = 71.43% yield}