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.

as given the equation is

2al + 6 hcl > 2 alcl3 + 3 h2(g)

as per equation two moles of aluminum reacts with six moles of hcl to give two moles of alcl3 and three moles of hydrogen gas

given: three moles of al are present and 7 moles of hcl

for three moles of aluminum nine moles of hcl will be required

however as 7 moles of hcl are present so the limiting reagent is hcl

hcl is going to decide the number of moles of product formed

when six moles of hcl are present = 3 moles of h2 are formed

when one mole of hcl is present == 3/6 mole sof h2 will be formed

when 7 moles of hcl are present = 3 x 7/ 6 moles of h2 will be formed = 3.5 moles of h2