Please, determine which reactant is limiting and what mass of each product is expected?

First we balance the equation:

S + 2H2SO4 -----> 3SO2 + 2H2O

We calculate the number of moles of each reactant by dividing 5.00g over the molar mass of the reactant

S = 32.1 g/mol
H2SO4 = 98.1 g/mol

moles of sulfur = 5.00g / 32.1g/mole = 0.156moles
moles of sulfuric acid = 5.00g / 98.1g/mol = 0.0510 moles

From the balanced equation we can see that ONE mole of sulfur reacts with TWO moles of sulfuric acid. Looking at the number of moles above, the limiting reactant is sulfuric acid.

0.051 moles of sulfuric acid (5.00g) reacts fully. We use the coefficients in the balanced equation to determine the following:
moles of SO2 expected = 0.0510moles x 3/2 = 0.0765moles
moles of H2O expected =  0.0510moles

We multiply the molar masses of the products with the number of moles to calculate their masses
mass of SO2 = 0.0765moles x 64.1g/mol = 4.90g
mass of H2O = 0.0510moles x 18.0g/mol = 0.918g

Hope that was clear and helpful.. Good luck!! =)