Sulfur dioxide gas (SO2) reacts with excess oxygen gas (O2) and excess liquid water (H2O) to form liquid sulfuric acid (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.
(One mole of any gas occupies 22.4 L under certain conditions of temperature and pressure. Assume those conditions for this question.)

Question

Sulfur dioxide gas (SO2) reacts with excess oxygen gas (O2) and excess liquid water (H2O) to form liquid sulfuric acid (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.
(One mole of any gas occupies 22.4 L under certain conditions of temperature and pressure. Assume those conditions for this question.)

minimato · Answer

So far I have the first part, and I know how to do the third part, but I can't do the third part without the second part, and I don't know how to solve that one. Can I get some help, please?

joannablackwelder · Answer

You can calculate the theoretical yield by using stoichiometry.

joannablackwelder · Answer

You are given that you have excess O2 and H2O, so the reaction would only be limited by the amount of SO2.

joannablackwelder · Answer

The only other piece of information you need besides what you are given and the balanced equation, is the molecular mass os sulfuric acid.

joannablackwelder · Answer

Make sense?