Type the correct answer in the box. express your answer to three significant figures. this balanced equation shows the reaction of sodium hydroxide and sulfuric acid: 2naoh + h2so4 → na2so4 + 2h2o. in a laboratory experiment, a student mixes 355 grams of sulfuric acid with an excess of sodium hydroxide. what is the theoretical mass of sodium sulfate produced? refer to the periodic table and the polyatomic ion resource. the theoretical mass of sodium sulfate is grams.

514.5 g.

Explanation:

n of H₂SO₄ = mass/molar mass = (355.0 g)/(98.0 g/mol) = 3.622 mol.

Using cross multiplication:

∵ 1.0 mol H₂SO₄ produces → 1.0 mol of Na₂SO₄.

∴ 3.622 mol H₂SO₄ produces → 3.662 mol of Na₂SO₄.

∴ mass of Na₂SO₄ =  no. of moles x molar mass = (3.662 mol)(142.04 g/mol) = 514.5 g.

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.