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2 April, 14:08

2. At STP, how many liters of oxygen are required to react completely with 3.6 liters

of hydrogen to form water?

2H2 (g) + O2 (g)

2H20 (g)

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Answers (1)
  1. 2 April, 15:34
    0
    1.8 L.

    Explanation:

    The balanced equation for the mentioned reaction is:

    2H₂ (g) + O₂ (g) → 2H₂O (g),

    It is clear that 2.0 moles of H₂ react with 1.0 mole of O₂ to produce 2.0 moles of H₂O.

    At STP, 3.6 L of H₂ reacts with (? L) of oxygen gas:

    It is known that at STP: every 1.0 mol of any gas occupies 22.4 L.

    using cross multiplication:

    1.0 mol of H₂ represents → 22.4 L.

    ? mol of H₂ represents → 3.6 L.

    ∴ 3.6 L of H₂ represents = (1.0 mol) (3.6 L) / (22.4 L) = 0.1607 mol.

    To find the no. of moles of O₂ nneded to react completely with 3.6 liters (0.1607 mol) of hydrogen:

    Using cross multiplication:

    2.0 mol of H₂ react completely with → 1.0 mol of O₂, from stichiometry.

    0.1607 mol of H₂ react completely with →? mol of O₂.

    ∴ The no. of moles of O₂ = (1.0 mol) (0.1607 mol) / (2.0 mol) = 0.08036 mol.

    Again, using cross multiplication:

    1.0 mol of O₂ represents → 22.4 L, at STP.

    0.08036 mol of O₂ represents →? L.

    ∴ The no. of liters of O₂ will be produced = (0.08036 mol) (22.4 L) / (1.0 mol) = 1.8 L.
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