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The chemical reaction in this example is of environmental interest. Iron pyrite (Fesz) is often an impurity in
coal, and so burning this fuel in a power plant produces sulfur dioxide (SO), a major air pollutant.
Calculate the mass of sulfur dioxide (SO2) produced when 3.84 mol O2 is reacted with Fes, according to the
equation
4 FeSacs + 11 O.
- 2 Fe2O3(-) + S SO2(e)

Respuesta :

178.87 grams of sulphur dioxide is formed according to the  equation given.

Explanation:

The balanced chemical reaction for the process is:

4 FeS2 + 11 O2 ⇒ 2Fe2O3(-) + 8 SO2

the reaction involving FeS and oxygen having balanced chemical equation as:

moles of oxygen given as 3.84

so when  11 moles of O2 reacts to form 8 moles SO2

                3.84 moles of oxygen reacts to form x moles of SO2

[tex]\frac{8}{11}[/tex] = [tex]\frac{x}{3.84}[/tex]

x = [tex]\frac{30.72}{11}[/tex]

2.792 moles of sulphur dioxide will be formed

The mass can be calculated as number of moles x molar mass of 1 mole of SO2

= 2.792 x 64.066

= 178.87 grams of sulphur dioxide is formed.

             

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