Question

A source of zinc metal can be zinc ore containing zinc(II) sulfide. The ore is roasted in pure oxygen to produce the oxide and then reduced with carbon to form elemental zinc and carbon monoxide. 2 ZnS + O2 2 ZnO + 2 SO2 ZnO + C Zn + CO A crucible containing a sample of 0.50 mol ZnS was roasted in pure oxygen, then reduced with 1.00 mol carbon. What mass remained in the crucible after cooling?

Answer 1

Answer:

32.7 grams of Zn will remained in the crucible after cooling.

Explanation:

$2ZnS+3O_2 \rightarrow 2ZnO + 2SO_2$..[1]

$ZnO+C\rightarrow Zn+CO$..[2]

Adding [1] + 2 × [2] we get:

$2ZnS+3O_2+2C \rightarrow 2Zn + 2CO+2SO_2$..[3]

Moles of ZnS in crucible = 0.50 mol

According to reaction [3]. 2 moles of ZnS gives 2 moles of Zn.

Then 0.50 moles of ZnS will give:

$\frac{2}{2}\times 0.50 mol=0.50 mol$ of Zn.

Mass of 0.50 moles of Zn =

= 0.50 mol × 65.4 g/mol =32.7 g

32.7 grams of Zn will remained in the crucible after cooling.