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12 August, 01:13

If 1.320 moles of CH4 reacts completely with oxygen, how many grams of H2O can be formed

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Answers (2)
  1. 12 August, 01:15
    0
    mass H2O = 47.56 g

    Explanation:

    balanced reation:

    CH4 + 2O2 → CO2 + 2H2O

    ∴ moles CH4 = 1.320 mol

    ⇒ moles H2O = (1.320 mol CH4) * (2 mol H2O/mol CH4)

    ⇒ moles H2O = 2.64 mol H2O

    ∴ molar mass (mm) H2O = 18.015 g/mol

    ⇒ mass H2O = (2.64 mol H2O) * (18.015 g/mol)

    ⇒ mass H2O = 47.56 g
  2. 12 August, 01:28
    0
    47.5 g of water can be formed

    Explanation:

    This is the reaction:

    CH₄ + 2O₂ → CO₂ + 2H₂O

    Methane combustion.

    In this process 1 mol of methane react with 2 moles of oxygen to produce 2 moles of water and 1 mol of carbon dioxide.

    As ratio is 1:2, I will produce the double of moles of water, with the moles of methane I have.

    1.320 mol. 2 = 2.64 moles

    Now, we can convert the moles to mass (mol. molar mass)

    2.64 mol. 18g/mol = 47.5 g
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