Chapter 3: Q154CP (page 139)

Sulfur dioxide is a major industrial gas used primarily for the production of sulfuric acid, but also as a bleach and food preservative. One way to produce it is by roasting iron pyrite (iron disulfide, FeS₂) in oxygen, which yields the gas and solid iron(III) oxide. What mass of each of the other three substances is involved in producing 1.00 kg of sulfur dioxide?

Short Answer

Expert verified

The mass of each of the other three substances are 936 g FeS₂, 687 g O₂ and 623 g Fe₂O₃.

Step by step solution

Calculating the moles of SO2

The chemical equation can be denoted as,

$4 F e S_{2} (s) + 11 O_{2} (g) \to 2 F e_{2} O_{3} (s) + 8 S O_{2} (g)$

On calculating the moles,

$\begin{array}{rcl} M o l e s o f S O_{2} & = & 1 \times 10^{3} g S O_{2} \times \frac{1 m o l S O_{2}}{64.06 g S O_{2}} \\ = & 15.6104 m o l S O_{2} \end{array}$

Calculating the mass of each elements

On finding the mass of each element,

$M a s s o f F e S_{2} = 15.6104 m o l S O_{2} \times \frac{4 m o l F e S_{2}}{8 m o l S O_{2}} \times \frac{119.98 g F e S_{2}}{1 m o l F e S_{2}} M a s s o f F e S_{2} = 936 g M a s s o f O_{2} = 15.6104 m o l S O_{2} \times \frac{11 m o l O_{2}}{8 m o l S O_{2}} \times \frac{32 g O_{2}}{1 m o l O_{2}} M a s s o f O_{2} = 687 g M a s s o f F e_{2} O_{3} = 15.6104 m o l S O_{2} \times \frac{2 m o l F e_{2} O_{3}}{8 m o l S O_{2}} \times \frac{159.69 g F e_{2} O_{3}}{1 m o l F e_{2} O_{3}} M a s s o f F e_{2} O_{3} = 623 g$