When solutions of H₂SO₄ and NaOH react, the balanced molecular equation is as follows: H₂SO₄(aq) + 2NaOH(aq) → Na₂SO₄(aq) + 2H₂O(l)
How much Na₂SO₄ is obtained when 4.00 g of H₂SO₄ reacts with 2.00 g of NaOH?

Question

Quizplus · Accepted Answer

To solve this problem, we need to use stoichiometry and convert the given masses of H₂SO₄ and NaOH to moles, then use the balanced equation to determine the mole ratio between the two compounds, and finally convert the resulting moles of Na₂SO₄ to grams. Molar mass of H₂SO₄ = 98.08 g/mol Molar mass of NaOH = 40.00 g/mol Number of moles of H₂SO₄ = 4.00 g / 98.08 g/mol = 0.0408 mol Number of moles of NaOH = 2.00 g / 40.00 g/mol = 0.0500 mol From the balanced equation, we see that the mole ratio between H₂SO₄ and Na₂SO₄ is 1:1. This means that 0.0408 mol of H₂SO₄ will react completely with 0.0408 mol of NaOH, leaving 0.0092 mol of NaOH in excess. The number of moles of Na₂SO₄ produced can be calculated from the mole ratio: 0.0408 mol H₂SO₄ x (1 mol Na₂SO₄ / 1 mol H₂SO₄) = 0.0408 mol Na₂SO₄ Finally, we can convert the moles of Na₂SO₄ to grams: 0.0408 mol Na₂SO₄ x 244.26 g/mol = 9.94 g However, we need to remember that although the balanced equation suggests Na₂SO₄ is a product, it may not provide us with the highest yield. To find the actual yield of Na₂SO₄, we need information about the reaction conditions such as concentration, temperature, reaction time, etc.

When Solutions of H2SO4 and NaOH React, the Balanced Molecular

When Solutions of H₂SO₄ and NaOH React, the Balanced Molecular