Question

when 1.0 m aqueous solutions of sodium carbonate and hydrochloric acid react it produces a carbon dioxide, water and sodium chloride (2 points) a.write the balanced chemical equation for the reaction described above (include states of matter) b.calculate the number of moles of carbon dioxide formed if 23.1 ml of sodium carbonate reacts with excess hydrochloric acid.

Answer 1

#a. Na₂CO₃(aq) + 2HCl (aq) → 2NaCl(aq) + CO₂(g) + H₂O(l)

#b. 0.0231 moles CO₂

Step-by-step explanation:

1. Carbonates reacts with acid to produce carbon dioxide and water as products.

• The reaction between sodium carbonate and hydrochloric acid yields sodium chloride, carbon dioxide and water.

The balanced equation for the reaction is;

Na₂CO₃(aq) + 2HCl (aq) → 2NaCl(aq) + CO₂(g) + H₂O(l)

Part B

• We are required to calculate the number of moles of CO₂ if 23.1 ml of Na₂CO₃ were used.

First, we need to calculate the number of moles of Na₂CO₃

• Volume of Na₂CO₃ is 23.1 mL or 0.0231 moles
• Molarity of concentration of Na₂CO₃ is 1.0 M

But;

Number of moles = Volume × Concentration

Therefore;

Moles of Na₂CO₃ = 0.0231 L× 1.0

= 0.0231 moles Na₂CO₃

Second, we can determine the moles of CO₂ produced.

• From the equation 1 mole of Na₂CO₃ reacts with the acid to produce 1 mole of CO₂.

This means, the mole ratio of Na₂CO₃ : CO₂ is 1 : 1

Therefore; Moles of CO₂ produced is 0,0231 moles

= 0.0231 moles CO₂