Molar mass of Fe2O3,
MM = 2*MM(Fe) + 3*MM(O)
= 2*55.85 + 3*16.0
= 159.7 g/mol
mass(Fe2O3)= 20.0 g
use:
number of mol of Fe2O3,
n = mass of Fe2O3/molar mass of Fe2O3
=(20 g)/(1.597*10^2 g/mol)
= 0.1252 mol
Molar mass of Al = 26.98 g/mol
mass(Al)= 2.0 g
use:
number of mol of Al,
n = mass of Al/molar mass of Al
=(2 g)/(26.98 g/mol)
= 7.413*10^-2 mol
Balanced chemical equation is:
Fe2O3 + 2 Al ---> 2 Fe + Al2O3
1 mol of Fe2O3 reacts with 2 mol of Al
for 0.1252 mol of Fe2O3, 0.2505 mol of Al is required
But we have 7.413*10^-2 mol of Al
so, Al is limiting reagent
we will use Al in further calculation
Molar mass of Fe = 55.85 g/mol
According to balanced equation
mol of Fe formed = (2/2)* moles of Al
= (2/2)*7.413*10^-2
= 7.413*10^-2 mol
use:
mass of Fe = number of mol * molar mass
= 7.413*10^-2*55.85
= 4.14 g
Answer: 4.14 g
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