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.

Zns + H2SO4aq                ZnSO4aq + H2g
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 = 4998=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 = 65 × 322161 = 130 g

Hope this information will clear your doubt regarding stoichiometry.

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