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Question

Find the moles of HCl gas obtained at STP from the following set of reactions:
FeCl3+O2Fe2O3+Cl2(g)H2(g)+Cl2(g)2HCl(g)
Starting with 4.56 mol of FeCl3 , 33.6 L of O2 at STP and 7 mol of H2 gas.
(Molar mass of Fe = 56 g/mol)


A
2 mol
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B
4 mol
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C
6 mol
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D
8 mol
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Solution

The correct option is C 6 mol
Balancing the given equation:
2FeCl3+32O2Fe2O3+3Cl2(g)H2(g)+Cl2(g)2HCl(g)
Moles of O2=given volume at STPmolar volume at STP=33.622.4=1.5 mol

Finding limiting reagent:
For FeCl3=Given molesstoichiometric coefficient=4.562=2.28For O2=given molesstoichiometric coefficient=1.51.5=1.0
So, oxygen will be the limiting reagent.
According to stoichiometry,
1.5 mol of O2 produces 3 mol of Cl2 gas.
In reaction (ii),
Finding the limiting reagent:
For H2=Given molesstoichiometric coefficient=71=7 molFor Cl2=Given molesstoichiometri coefficient=31=3 mol
So, chlorine will be the limiting reagent.
1 mol of Cl2 produces 2 mol of HCl.
3 mol will produce 6 mol of HCl.

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