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ChemistryNumerical+4Question 34 of 54

JEE Advanced 2020 · Paper 1, Chemistry question 16

Aluminium reacts with sulfuric acid to form aluminium sulfate and hydrogen. What is the volume of hydrogen gas in liters (L) produced at 300 K and 1.0 atm pressure, when 5.4 g of aluminium and 50.0 mL of 5.0 M sulfuric acid are combined for the reaction?

(Use molar mass of aluminium as 27.0 g mol−127.0\ \mathrm{g\,mol^{-1}}, R=0.082 atm L mol−1 K−1R = 0.082\ \mathrm{atm\,L\,mol^{-1}\,K^{-1}})

Answer and worked solution

Official answer: 6

Reaction. 2 Al+3 HX2SOX4→AlX2(SOX4)X3+3 HX2\ce{2Al + 3H2SO4 -> Al2(SO4)3 + 3H2}.

Amounts.

  • Al: 5.4/27=0.205.4/27=0.20 mol.
  • HX2SOX4\ce{H2SO4}: 0.050×5.0=0.250.050\times5.0=0.25 mol.

0.20 mol Al would need 0.30 mol acid, so the acid is limiting. It gives 0.25 mol HX2\ce{H2}.

Volume.
V=nRTP=0.25×0.082×3001.0=6.15 L.V=\frac{nRT}P=\frac{0.25\times0.082\times300}{1.0}=6.15\text{ L}.
Answer: 6.15 (key: 6.00 to 6.20)

Topics:StoichiometryIdeal gas equation
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