Q154CP

Question

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?

Step-by-Step Solution

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Answer

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

1Step 1: Calculating the moles of SO 2

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,

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

2Step 2: Calculating the mass of each elements

On finding the mass of each element,

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

Q153CP

Q155CP

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