H2SO4). In the laboratory, a chemist carries out this reaction with 67.2 L of sulfur dioxide and gets 250 g of sulfuric acid. • Write a balanced equation for the reaction. • Calculate the theoretical yield of sulfuric acid. • Calculate the percent yield of the reaction.

Question

H2SO4). In the laboratory, a chemist carries out this reaction with 67.2 L of sulfur dioxide and gets 250 g of sulfuric acid. •	Write a balanced equation for the reaction. •	Calculate the theoretical yield of sulfuric acid. •	Calculate the percent yield of the reaction.

alphadxg · Answer

2 SO2 + O2 + 2 H2O → 2 H2SO4 

(67.2 L SO2) / (22.4 L/mol) x (2 mol H2SO4 / 2 mol SO2) x 
(98.0791 g H2SO4/mol) = 294 g H2SO4 

(250 g) / (294 g) = 0.850 = 85.0% yield

Also you have to remember that (One mole of any gas occupies 22.4 L under certain conditions of temperature and pressure. Assume those conditions for this question.)