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Question

Which of the following statement(s) is/are incorrect when 0.15 mol of Fe is allowed to react with 4.8 g of O2?
(Molar mass of Fe=56 g/mol)
4Fe(s)+3O2(g)2Fe2O3(s)

A
Fe is the limiting reagent
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B
The mass of O2 left over at the end of the reaction is 1.2 g
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C
The mass of Fe2O3 produced is 12.0 g
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D
O2 is the limiting reagent
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Solution

The correct option is D O2 is the limiting reagent
4Fe+3O22Fe2O3
Moles of O2=4.832=0.15 mol

Finding the limiting reagent,
For Fe=given moles stoichiometric coefficient=0.154=0.0375
For O2=given moles stoichiometric coefficient=0.153=0.05

So, Fe is the limiting reagent.

4 mol of Fe react with 3 mol of O2
0.15 mol of Fe will react with, 34×0.15=0.1125 moles of O2

Amount of O2 reacted = 0.1125×32=3.6 g
Amount of O2 left = 4.83.6=1.2 g

4 moles of Fe produces 2 moles of Fe2O3
Molar mass of Fe2O3=56×2+3×16=160 g/mol
0.15 mol will produce 2×0.154 = 0.075 mol of Fe2O3

Amount of Fe2O3=0.075×160=12 g
O2 is the excess reagent.
Therefore, option (d) is the incorrect statement.

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