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JEE MainChemistrySome Basic Concepts of Chemistry

A 0.54 g sample of aluminium reacts completely with an excess of dilute hydrochloric acid. The volume of hydrogen gas evolved at STP is: (Given: Molar mass of Al = 27 g mol ⁻¹ , Molar volume of a gas at STP = 22.4 L mol ⁻¹ )

Options

  1. A672 mL
  2. B448 mL
  3. C1344 mL
  4. D0.672 mL

Correct answer

A. 672 mL

Step-by-step solution

The balanced chemical equation for the reaction is: 2 Al + 6 HCl 2 AlCl ₃ + 3 H ₂ Moles of Al reacted = 0.54 27 = 0.02 mol From the stoichiometry of the reaction, 2 moles of Al produce 3 moles of H ₂ . Moles of H ₂ produced = 3 2 0.02 = 0.03 mol Volume of H ₂ at STP = 0.03 mol 22.4 L mol ⁻¹ = 0.672 L Converting to mL: Volume = 0.672 1000 = 672 mL Answer: 672 mL

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