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Lead can be prepared from galena [lead(ii) sulfide] by first roasting the galena in oxygen gas to form lead(ii) oxide and sulfur dioxide. Heating the metal oxide with more galena forms the molten metal and more sulfur dioxide.

Required:
a. Write a balanced equation for each step.
b. Write an overall balanced equation for the process.
c. How many metric tons of sulfur dioxide form for every metric ton of lead obtained?

Respuesta :

potatosuspotato

Answer:

I don't really have an answer it's very confusing sorry

Explanation:

... ;w;

a. The balanced chemical equation of all steps mention in question.

1. [tex]2PbS(s) + 3O_{2}(g)[/tex] → [tex]2PbO(s) + 2SO_{2}(g)[/tex]

2.[tex]2PbO(s) + PbS_{}(s)[/tex] → [tex]3Pb(l) + SO_{2}(g)[/tex]

b. An overall balanced equation for the process.

[tex]PbS(s) + O_{2}(g)[/tex] → [tex]Pb(l) + SO_{2}(g)[/tex]

c. 0.31 metric tons of [tex]sulfur dioxide[/tex] form for every metric ton of [tex]lead[/tex]obtained.

One metric ton of [tex]lead[/tex] obtained = 1×[tex]10^{6}[/tex]g of [tex]Pb[/tex]

Molar mass of [tex]Pb[/tex] = 207.2 g/mol

Moles of [tex]SO_{2}[/tex] = 1×[tex]10^{6}[/tex] g of [tex]Pb[/tex] × 1 mol [tex]Pb[/tex]/207.2 g of [tex]Pb[/tex] × 1 mol [tex]SO_{2}[/tex] /1 mol [tex]Pb[/tex] = 4826.25 moles [tex]SO_{2}[/tex]

Molar mass of [tex]SO_{2}[/tex] = 64.07 g/mol

Mass of [tex]SO_{2}[/tex] formed = 4826.25 mol [tex]SO_{2}[/tex] × 64.07 g [tex]SO_{2}[/tex]/1 mol [tex]SO_{2}[/tex] = 3.09 × [tex]10^{5}[/tex]  g [tex]SO_{2}[/tex]

Mass of [tex]SO_{2}[/tex] formed = 0.31 matric ton [tex]SO_{2}[/tex].

What is chemical equation?

The symbolic representation of conversion reactant into product is called chemical equation.

To learn more about chemical equation here.

https://brainly.com/question/12047033

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