Question

When 107 g NaCl (MM=58.44 g/mol) and 135 g H₂SO₄ (MM=98.08 g/mol) are mixed and react according to the equation below, what is the mass in grams (g) of Na₂SO₄ produced? Give your answer rounded to a whole number. Do not enter units. (Hint: Find the limiting reactant; Na₂SO₄=142.04 g/mol)

2NaCl + H₂SO₄→ Na₂SO₄ + 2HCl

Answer 1

The mass of Na₂SO₄ produced is 130 g.

Step-by-step explanation:

To find the mass of Na₂SO₄ produced, we first need to determine the limiting reactant. We can do this by comparing the number of moles of each reactant.

For NaCl:

Number of moles = mass / molar mass = 107 g / 58.44 g/mol = 1.83 mol

For H₂SO₄:

Number of moles = mass / molar mass = 135 g / 98.08 g/mol = 1.38 mol

We can see that NaCl has a greater number of moles, which means it is the limiting reactant.

Using the balanced equation, we can see that 2 moles of NaCl reacts to produce 1 mole of Na₂SO₄.

Therefore, the number of moles of Na₂SO₄ produced = 1.83 mol NaCl * (1 mol Na₂SO₄ / 2 mol NaCl) = 0.915 mol

To find the mass of Na₂SO₄ produced, we multiply the number of moles by the molar mass:

Mass = number of moles * molar mass = 0.915 mol * 142.04 g/mol

= 129.98 g

Rounding this to the nearest whole number, the mass of Na₂SO₄ produced is 130 g.