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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.

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superman1987

Answer:

514.5 g.

Explanation:

  • The balanced equation of the reaction is: 2NaOH + Hâ‚‚SOâ‚„ → Naâ‚‚SOâ‚„ + 2Hâ‚‚O.
  • It is clear that every 2.0 moles of NaOH react with 1.0 mole of Hâ‚‚SOâ‚„ to produce 1.0 mole of Naâ‚‚SOâ‚„ and 2.0 moles of 2Hâ‚‚O.
  • Since NaOH is in excess, so Hâ‚‚SOâ‚„  is the limiting reactant.
  • We need to calculate the no. of moles of 355.0 g of Hâ‚‚SOâ‚„:

n of Hâ‚‚SOâ‚„ = 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.

  • Now, we can get the theoretical mass of Naâ‚‚SOâ‚„:

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

Answer:

its 514

Explanation:

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