A sample of 0.7 moles of metal 'M' reacts completely with an excess of fluorine to form 45g of MF2. How many moles of F are present in it?
Correct answer: A. 1.4 moles
- A. 1.4 moles
- B. 2.4 moles
- C. 2 moles
- D. 1.2 moles
Explanation
1 mole of metal formed one mole of MF2 molecule ∴ 0.7 mole of metal formed = 0.7 mole MF2 molecule ∵ Each molecule of MF2 contains = 2F atoms ∴ 0.7 mole of MF2 molecule contains = 2 x 0.7 moles of F atom = 1.4 mole of F atom Hence, 45 g of MF2 molecule contains 1.4 moles 'F' atom.
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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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