Question

part a
for the reaction, calculate how many grams of the product form when 2.6 g of cl₂ completely reacts. assume that there is more than enough of the other reactant.
2 na(s) + cl₂(g) → 2 nacl(s)
express your answer using two significant figures.
part b
for the reaction, calculate how many grams of the product form when 2.6 g of cao completely reacts. assume that there is more than enough of the other reactant.

Explanation:

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

Molar mass of \( \text{Cl}_2 \) is \( 2\times35.45 = 70.90 \, \text{g/mol} \). Moles of \( \text{Cl}_2 = \frac{2.6 \, \text{g}}{70.90 \, \text{g/mol}} \approx 0.0367 \, \text{mol} \).

Step2: Use stoichiometry

From reaction \( 2\text{Na} + \text{Cl}_2
ightarrow 2\text{NaCl} \), 1 mol \( \text{Cl}_2 \) produces 2 mol \( \text{NaCl} \). So moles of \( \text{NaCl} = 2\times0.0367 = 0.0734 \, \text{mol} \).

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

Molar mass of \( \text{NaCl} = 22.99 + 35.45 = 58.44 \, \text{g/mol} \). Mass of \( \text{NaCl} = 0.0734 \, \text{mol} \times 58.44 \, \text{g/mol} \approx 4.3 \, \text{g} \).

Answer:

\( 4.3 \)