Question

Sulfurous acid is unstable in aqueous solution and gradually decomposes to water and sulfur dioxide gas (which explains the choking odor associated with sulfurous acid solutions) H2SO3 (ag)H20()SO2 (g) If 7.20 g of sulfurous acid undergoes this reaction, what mass of sulfur dioxide is released? g SO2

Answer 1

From balanced chemical equation we can see the number of moles of product formed from the number of moles of species get reacted and from the relation of their number of moles of reactant reacted or number of moles of product formed we can calculate their amount in gram.

Solution As the reaction is balanced, we can stoichiometric relationship H, SQ3 (29) -> H2O(l) +50,7). It means 1 mole H Solaal de compses to give 1 mole of So, (g). 1 mole H, SO (ar) - 1 mole sog) bet ng of so Mole Number of t. so reacts = giren mass molecular mass 7. 20 82.07 = 0.087 or 0.09 As 1 mole H, so gives 1 mol so Therefore 0.09 mole of H₂SO3 will give 0.09 mole of sor. number of mole of so, produced=0.09 given mass, molecular mass=0.09. → mass of SO2-0.09 Now, mass of so, produced = 64.06680-og 64.066 = 5.76 g.