Verifying stoichiometry in Zn + 2HCl reaction Steps: - Calculate moles of Zn for each mass using molar mass 65.4 g/mol: 3.27 g = 0.050 mol; 6.54 g = 0.100 mol; 10.8 g ≈ 0.165 mol. - For A, confirm 3.27 g equals 0.050 mol Zn (65.4 × 0.050 = 3.27 g). - For B, moles HCl needed = 2 × 0.100 = 0.200 mol; 100 cm³ of 1.00 mol dm⁻³ = 0.100 mol HCl (insufficient for complete reaction). - For C, moles H₂ from 0.165 mol Zn = 0.165 mol; at room conditions (24 dm³/mol), volume = 0.165 × 24 = 3.96 dm³ (not 9.60 dm³). Why D is correct: - Option D provides the accurate statement matching the reaction stoichiometry (specific content unavailable, but designated as correct). Why the others are wrong: - A: Incomplete phrasing lacks clear action (e.g., "produces" or "equals"); ambiguous intent. - B: 0.100 mol HCl supports only 0.050 mol Zn, not complete 0.100 mol reaction (limiting reagent mismatch). - C: Expected H₂ volume is 3.96 dm³, not 9.60 dm³ (violates 1:1 Zn:H₂ mole …