Question

Use the References to access important values if needed for this question. It is desired to produce 6.30 grams of sulfurous acid (H2SO3) by the following reaction. If the percent yield of sulfurous acid (H2S03) is 75.6 %, how many grams of sulfur dioxide would need to be reacted? gras sulfur dioxide sulfur dioxide(g) + water(l) — sulfurous acid (H2SO3)(g)

Answer 1

+ - SO2 64ginal H2O 18 ginos H2SO3 82 gimol MW = : moles of H2SO3 produced = = 0.0768 3 mol 6.30 g 82 gimol 1 mol s02 produces 1 mol H2SO3 . . : Theoretical yield = Actorsual yreld X100 % yield 0.07683 mol X 100 75.6 = 0.101626 mol mass of SO2 rearted = 0.101626 mol x64 g (mol T= 6.50 g h Xe + 2F2 Tånitial 2 6 ofined - 2 Xefu - 2 Limiting reagent is [Xeb is [2l, and to the no. of the no. of Xe Fu Molecules formed F2/molecules in excess is [2.