Question

An alloy of iron and carbon was treated with sulfuric acid, in which only the iron...

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)

Homework Answers

Answer #1

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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