Answer to Question #199108 in Chemistry for jordan

Question

4. Calcium carbonate (CaCO3) which is found in limestone and marble reacts readily with hydrochloric acid (HCl) to produce calcium chloride (CaCl2), carbon dioxide, and water.

a. Write the balanced chemical reaction:

b. What mass of hydrochloric acid will be needed to produce 325 g of calcium chloride?

c. What mass of carbon dioxide could be produced if 750 g of calcium carbonate reacts with excess hydrochloric acid?

Answer 1

Solution:

a)

Balanced chemical equation:

CaCO₃(s) + 2HCl(aq) → CaCl₂(aq) + CO₂(g) + H₂O(l)

b)

The molar mass of HCl is 36.458 g/mol.

The molar mass of CaCl₂ is 110.98 g/mol.

According to the equation above: n(HCl)/2 = n(CaCl₂)

Therefore,

(325 g CaCl₂) × (1 mol CaCl₂ / 110.98 g CaCl₂) × (2 mol HCl / 1 mol CaCl₂) × (36.458 g HCl / 1 mol HCl) = 213.53 g HCl

c)

The molar mass of CaCO₃ is 100.087 g/mol.

The molar mass of CO₂ is 44.01 g/mol.

According to the equation above: n(CaCO₃) = n(CO₂)

Therefore,

(750 g CaCO₃) × (1 mol CaCO₃ / 100.087 g CaCO₃) × (1 mol CO₂ / 1 mol CaCO₃) × (44.01 g CO₂ / 1 mol CO₂) = 329.79 g CO₂

Answers:

a) CaCO₃(s) + 2HCl(aq) → CaCl₂(aq) + CO₂(g) + H₂O(l)

b) 213.53 g HCl

c) 329.79 g CO₂