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Stoichiometric Calculations

Find the volu...

Question

Find the volume of hydrogen which would be evolved at STP by reacting zinc with $50$ mL of $40 %$ pure dil. $H_{2} S O_{4}$ (density= $1.3$ g/mL ). Report your answer in litres, rounded to the nearest integer.

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Solution

The balanced chemical equation is as given below
$Z n + H_{2} S O_{4} \to Z n S O_{4} + H_{2}$
Here, we assume that sulfuric acid is the limiting reagent.
The mass of sulfuric acid is $50$ mL $\times 1.3$ g/mL $\times 0.4 = 26$ g $H_{2} S O_{4}$ .
The number of moles of sulphuric acid is $\frac{26}{98} = 0.265$ mol.
Equal number of moles of hydrogen will be produced.
The volume of hydrogen produced at STP will be $0.265$ mol $\times 22.4$ L $= 5.94$ L $= 6$ L.

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