Answer
2.46 kg $O_{2}$.
Work Step by Step
Balanced chemical reaction:
2ZnS(s) +3 $O_{2}$ (l)${\longrightarrow}$ 2 ZnO +2 $SO_{2}$ (g)
The strategy to find the mass of $O_{2}$ that react with 5.0 x $10^{3}$ g ZNS is:
g ZnS ${\rightarrow}$ mol ZnS ${\rightarrow}$ mol $O_{2}$${\rightarrow}$ g $O_{2}$
The conversion factors are:
$\frac{1 mol ZnS}{Molar mass (ZnS)}$ to convert to moles ZnS, where Molar mass ZnS:
Molar mass ZnS= 1 x 65.4 g + 1 x32.0 = 97.4 g
$\frac{3 mol (O_{2})}{2 mol (ZnS)}$, to convert the moles of ZnS to mol of $O_{2}$.
$\frac{Molar mass(O_{2)}}{1 mol(O_{2})}$ to convert to g of $O_{2}$, where the molar mass of $O_{2}$ is:
molar mass of $O_{2}$= 2 x 16=32 g
Now we use of the conversion factors to find the mass of $O_{2}$:
5.0 x $10^{3}$ g ZNS x $\frac{1 mol ZnS}{Molar mass (ZnS)}$ x $\frac{3 mol (O_{2})}{2 mol (ZnS)}$ x $\frac{Molar mass(O_{2)}}{1 mol(O_{2})}$ =
5.0 x $10^{3}$ g ZNS x $\frac{1 mol ZnS}{97.4 g (ZnS)}$ x $\frac{3 mol (O_{2})}{2 mol (ZnS)}$ x $\frac{32.0 g(O_{2)}}{1 mol(O_{2})}$ = 2.46 x $10^{3}$ g $O_{2}$ or 2.46 kg $O_{2}$ .
