What mass of sulphuric acid will be required to produce hydrogen that will reduce 8.5 g of
copper oxide to metallic copper?
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11th
Chemistry
Some Basic Concepts of Chemistry
Stoichiometry and Stoichiometric Calculations
What weight of zinc would b...
CHEMISTRY
What weight of zinc would be required to produce enough hydrogen to reduce 8.5 g of copper oxide completely into copper?
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Solution:-
Reaction of zinc to produce hydrogen-
Zn+2HCl⟶ZnCl
2
+H
2
Reaction of hydrogen to reduce copper oxide into copper-
CuO+H
2
⟶H
2
O+Cu
From the above reactions-
1 moles of Zn produces 1 mole of hydrogen gas and 1 mole of hydrogen required to reduce 1 mole of CuO.
Mole of CuO reduced = mole of Zn required
Therefore,
No. of moles of CuO reduced =
molar mass of CuO
moles of CuO
Given weight of CuO=8.5g
Molecular weight of CuO=79.5g
Therefore,
No. of moles of CuO reduced =
79.5
8.5
=0.107 mol
Therefore,
No. of moles of Zn required =0.107 mol
Now,
Molecular weight of Zn=65.4g
∴ Weight of Zn required =0.107×65.4=6.99g
Hence 6.99g of Zn will be required.
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