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The number of moles of Mg required to produce 11.212dm3 of Hydrogen at SIT when it reacts with HCl solution, are Mg + 2HCI MgCl2 + H2

Correct answer: C. 0.5 mole

  • A. 1 mole
  • B. 2 moles
  • C. 0.5 mole
  • D. 0.25 moles

Explanation

To find the number of moles of magnesium (Mg) required, consider the stoichiometry of the reaction: Mg + 2HCl → MgCl2 + H2. According to the ideal gas law, 1 mole of any gas at standard temperature and pressure (STP) occupies 22.4 dm3. Therefore, to produce 11.2 dm3 of hydrogen gas, 0.5 moles of Mg is required. Option C is correct. Option A suggests 1 mole of Mg, which would produce 22.4 dm3 of H2, double the required amount. Option B suggests 2 moles, producing an even larger volume of 44.8 dm3, and Option D suggests 0.25 moles, producing only 5.6 dm3 of H2, half of the required volume.

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About Fundamental Concepts of Chemistry

Mole calculations connect mass, number of particles and Avogadro's number, while balanced equations provide the mole ratios used in stoichiometry. Questions cover limiting and excess reactants, theoretical yield and percentage yield, including identifying which reactant is consumed first and comparing the actual product with the maximum possible product.

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