Consider the following reaction between zinc and dilute sulphuric acid.
Zn(s) + H₂SO₄(aq) gives ZnSO_​4(aq) + H₂(g)
Answer the following questions based on the above chemical equation.
(a) Name the type of chemical reaction.
(b) Calculate the volume at STP of hydrogen gas that would be produced when 49 g of sulphuric acid reacts completely with zinc.
(c) The mass of zinc that would be required to produce 322 g of zinc sulphate.
(Atomic mass : Zn = 65, S =32 , H = 1,0 = 16)

Dear student,

Please find below the solution to the query posted by you.

$\mathrm{Zn}\left(\mathrm{s}\right) + {\mathrm{H}}_2{\mathrm{SO}}_4\left(\mathrm{aq}\right) \stackrel{ }{\to } {\mathrm{ZnSO}}_4\left(\mathrm{aq}\right) + {\mathrm{H}}_2\left(\mathrm{g}\right)$
a. This reaction is an example of displacement reaction.

b. According to the balanced chemical reactions,

Moles of H₂ produced from 1 mole of H₂SO₄ = 1 mole
Moles of H₂SO₄ in 49 g = $\frac{49}{98}=0.5$
Moles of H₂ produced from 0.5 moles of H₂SO₄ = 0.5
Volume of H₂ in 0.5 moles, at STP = 0.5 ⨯ 22.4 L = 11.2 L

c. Mass of Zn required to produce 161 g of ZnSO_​4 = 65 g
Mass of Zn required to produce 322 g of ZnSO₄ = $\frac{65 \times 322}{161} = 130 \mathrm{g}$

Hope this information will clear your doubt regarding stoichiometry.

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