Problem
Given the balanced equation representing a reaction: \[ 2 \mathrm{NaCl}(\ell) \rightarrow 2 \mathrm{Na}(\ell)+\mathrm{Cl}_{2}(g) \] A 1170. -gram sample of \( \mathrm{NaCl}(\ell) \) completely reacts, producing 460. grams of \( \mathrm{Na}(\ell) \). What is the total mass of \( \mathrm{Cl}_{2}(\mathrm{~g}) \) produced? \( 1355 \mathrm{~g} \) 2. 710. \( g \) 3. 1420. \( g \) 4. \( 1630 . \mathrm{g} \)
Solution
Step 1 ：\( \frac{1170 \mathrm{g} \, \mathrm{NaCl}}{2 \mathrm{mol}} \times \frac{58.44\mathrm{g}}{1 \mathrm{mol}} \)
Step 2 ：\( \frac{460 \mathrm{g} \, \mathrm{Na}}{2 \mathrm{mol}} \times \frac{22.99\mathrm{g}}{1 \mathrm{mol}} \)
Step 3 ：\( 1170 \mathrm{g} - 460 \mathrm{g} = 710 \mathrm{g} \)
