Question

part d
for the reaction, calculate how many grams of the product form when 2.6 g of na₂o completely reacts.
assume that there is more than enough of the other reactant.
express your answer using two significant figures.
na₂o(s) + h₂o(l) → 2 naoh(aq)

Explanation:

Step1: Calculate moles of \( \text{Na}_2\text{O} \)

Molar mass of \( \text{Na}_2\text{O} \): \( 2\times22.99 + 16.00 = 61.98 \, \text{g/mol} \).
Moles of \( \text{Na}_2\text{O} = \frac{2.6 \, \text{g}}{61.98 \, \text{g/mol}} \approx 0.0419 \, \text{mol} \).

Step2: Relate moles of \( \text{Na}_2\text{O} \) to \( \text{NaOH} \)

From the reaction \( \text{Na}_2\text{O} + \text{H}_2\text{O}
ightarrow 2\text{NaOH} \),
1 mol \( \text{Na}_2\text{O} \) produces 2 mol \( \text{NaOH} \).
Moles of \( \text{NaOH} = 0.0419 \, \text{mol} \times 2 = 0.0838 \, \text{mol} \).

Step3: Calculate mass of \( \text{NaOH} \)

Molar mass of \( \text{NaOH} \): \( 22.99 + 16.00 + 1.01 = 40.00 \, \text{g/mol} \).
Mass of \( \text{NaOH} = 0.0838 \, \text{mol} \times 40.00 \, \text{g/mol} \approx 3.35 \, \text{g} \).
Round to two significant figures: \( 3.4 \, \text{g} \).

Answer:

\( 3.4 \)