Question

what volume of Hydrogen would be liberated when 11.2g of Iron Fe reacts with excess dilute tetraoxosulphate(vi) acid
H2SO4
H- 1 O-16 S-22 Fe- 36

Answer 1

Answer on Question #57540 - Chemistry - Inorganic Chemistry

Question:

what volume of Hydrogen would be liberated when 11.2g of Iron Fe reacts with excess dilute tetraoxosulphate(vi) acid

$$\mathrm{H_2SO_4}$$

H- 1 O-16 S-22 Fe- 36

Solution.

The reaction of excess dilute tetraoxosulphate(vi) acid with Iron

$$\mathrm{Fe} + \mathrm{H_2SO_4} = \mathrm{FeSO_4} + \mathrm{H_2}$$

Amount of moles of Iron

$$\frac{11.2\ \text{g}}{56\ \text{g/mol}} = 0.2\ \text{mol}$$

So, reacting of 0.2 moles of Iron forms 0.2 moles of Hydrogen which correspond to

$$0.2\ \text{mol} \times 22.4\ \frac{\text{l}}{\text{mol}} = 4.48\ \text{l}$$

Answer: 4.48 l

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