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. \( 1630 . \mathrm{g} \)

Answer

Expert–verified

Hide Steps

Answer

\( 1170 \mathrm{g} - 460 \mathrm{g} = 710 \mathrm{g} \)

Steps

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 ：\( 1170 \mathrm{g} - 460 \mathrm{g} = 710 \mathrm{g} \)