How many water molecules will be lost on completely dehydrating 0.684 g of sucrose (C₁₂H₂₂O₁₁)?
Correct answer: A. 1.32 x 10²²
- A. 1.32 x 10²²
- B. 6.02 x 10²⁰
- C. 6.62 x 10²¹
- D. 1.20 x 10²²
Explanation
First, find the moles of sucrose: 0.684 g / 342 g/mol = 0.002 mol. The dehydration reaction C₁₂H₂₂O₁₁ → 12C + 11H₂O shows 11 moles of water are produced per mole of sucrose, so 0.022 mol of water are formed. The number of molecules is 0.022 mol × (6.022 × 10²³ molecules/mol) ≈ 1.32 × 10²² molecules.
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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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