An alloy of iron and carbon was treated with sulfuric acid, in which only the iron reacts.
if a sample of alloy weighing 2.358g gave home hydrogen which causes an explosion and generated 1.0368g of water, what is the percencentage of iron in the alloy?
(hint: Hydrogen can react with oxygen in the air and explode)
The chemical reactions involved in the given process are
Dissolution: 2Fe + 3H2SO4 Fe2(SO4)3 +3H2
Explosion: 2H2 + O2 2H2O
Number of moles of H2O produced = weight/ molar mass = 1.0368 g / 18 .02 = 0.0575 mol
According to second equation, the mole ratio between H2 and H2O is 1:1
So, in the first step, 0.0575 mol of H2 is produced.
From the stochiometry of first equation, the molar ratio between Fe and H2 is 2:3.
So, amount of iron presnt in the sample = (2/3)* 0.0575 mol = 0.038 mol
Converting this into grams = 0.038 mol * 55.84 g/mol = 2.140 g
So, out of 2.358 g, 2.140g is iron.
The percentage of iron in the alloy = 90.75 %
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