Calculate the number of moles of Mg required to produce 11.212 dm3 of Hydrogen gas at STP when it reacts with HCl solution. The equation for this reaction is: Mg + 2HCl ---> MgCl2 + H2
Correct answer: C. 0.5 moles
- A. 1 mole
- B. 2 moles
- C. 0.5 moles
- D. 0.25 moles
Explanation
Moles of H2 to be produced: Mole = Volume / Volume at STP = 11.212 / 22.14 = 0.50mol According to the equation the ratio of moles of Mg and H2 is 1 : 1 so, moles of Mg = 0.50
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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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