Answer to Question #162376 in Chemistry for Ava Brooke

Question

Using the following chemical equation how many grams of water are produced by reacting 59.33 g of calcium hydroxide?

2HCl + Ca(OH)₂ -> 2H₂O + CaCl₂

Answer 1

Solution:

The balanced chemical equation:

Ca(OH)₂ + 2HCl → CaCl₂ + 2H₂O

According to the equation above: n(Ca(OH)₂) = n(H₂O)/2

Moles of Ca(OH)₂ = Mass of Ca(OH)₂ / Molar mass of Ca(OH)₂

The molar mass of Ca(OH)₂ is 74.093 g mol^-1.

Hence,

n(Ca(OH)₂) = 59.33 g / 74.093 g mol^-1 = 0.80075 mol

n(H₂O) = 2 × n(Ca(OH)₂) = 2 × 0.80075 mol = 1.6015 mol

Moles of H₂O = Mass of H₂O / Molar mass of H₂O

Mass of H₂O = Moles of H₂O × Molar mass of H₂O

The molar mass of H₂O is 18.0153 g mol^-1.

Hence,

m(H₂O) = 1.6015 mol × 18.0153 g mol^-1 = 28.8515 g = 28.85 g

Answer: 28.85 grams of water (H₂O) are produced.