Question

If 20 g of NaOH reacts with 30 g of H₂SO₄ to produce Na₂SO₄ according to the reaction below, how many grams of Na₂SO₄ are produced?

NaOH + H₂SO₄ → Na₂SO₄ + H₂O

Answer 1

The reaction between NaOH and H₂SO₄ produces Na₂SO₄, with H₂SO₄ being the limiting reactant. After calculating moles based on given masses, we find that 43.45 g of Na₂SO₄ are formed from the reaction of 20 g of NaOH with 30 g of H₂SO₄.

Step-by-step explanation:

To determine the mass of the product Na2SO4 formed in the reaction between NaOH and H2SO4, a stoichiometry calculation must be performed. The balanced chemical equation is H2SO4 (aq) + 2NaOH (aq) → Na2SO4 (aq) + 2H2O(l).

The molar mass of NaOH is approximately 40 g/mol, and H2SO4 is approximately 98 g/mol. First, calculate the moles of each reactant:

• 20 g NaOH * (1 mol / 40 g) = 0.5 mol NaOH
• 30 g H2SO4 * (1 mol / 98 g) = 0.306 mol H2SO4

Using the balanced equation, we need twice the amount (2:1 ratio) of NaOH for one mole of H2SO4, meaning H2SO4 is the limiting reactant. Thus:

• 0.306 mol H2SO4 * (1 mol Na2SO4 / 1 mol H2SO4) = 0.306 mol Na2SO4

Finally, to find the mass, use the molar mass of Na2SO4 (142 g/mol):

• 0.306 mol Na2SO4 * 142 g/mol = 43.45 g Na2SO4

Therefore, 43.45 g of Na2SO4 are produced.