2. 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.)

See explanation

Explanation:

The balanced equation for the formation of sulphuric acid is;

2SO2 + O2 + 2H2O → 2H2SO4

If 1 mole of SO2 occupies 22.4 L

x moles occupy 67.2 L

x = 1 × 67.2/22.4

x= 3 moles

From the reaction equation;

2 moles of SO2 yields 2 moles of H2SO4

Hence 3 moles of SO2 also yields 3 moles of H2SO4

Theoretical yield of H2SO4 = 3 moles × 98 g/mol = 294 g

Percent yield = actual yield/theoretical yield × 100

Percent yield = 250g/294g × 100

Percent yield = 85%

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !