Soru
Given the equation 2H_(2)Oarrow 2H_(2)+O_(2) how many moles of H_(2)O would be required to produce 80 g of O_(2) A. 1.0 mol B. 2.0 mol C. 4.0 mol D. 5.0 mol A B c D
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3.9
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İbrahim
Profesyonel · 6 yıl öğretmeni
Uzman doğrulaması
Cevap
To solve this problem, we need to use the concept of stoichiometry and the molar mass of oxygen (O2).Given information:- The balanced chemical equation is: 2H2O → 2H2 + O2- We need to find the number of moles of H2O required to produce 80 g of O2.Step 1: Calculate the molar mass of O2.Molar mass of O2 = 16.00 g/mol × 2 = 32.00 g/molStep 2: Calculate the number of moles of O2.Number of moles of O2 = 80 g / 32.00 g/mol = 2.5 molStep 3: Use the stoichiometric relationship between H2O and O2.According to the balanced equation, 2 moles of H2O are required to produce 1 mole of O2.Therefore, the number of moles of H2O required = 2 × 2.5 mol = 5.0 molTherefore, the correct answer is D. 5.0 mol.