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17 February, 09:30

2.0 g of H2 gas reacts with 32 g of O2 gas to form water. Assuming the reaction goes to completion, how many grams of water will be produced?

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  1. 17 February, 12:12
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    In order to solve this problem, the balanced chemical equation of the reaction must be used. This gives the equation:

    2H2 + O2 - - > 2H2O

    Next, the moles of the reactants must be used in order to apply their stoichiometric relationships. Note that 1 mole of oxygen needs 2 moles of hydrogen for the reaction proceed. Since there is only 1 mole of H2, only 0.5 moles of oxygen are consumed.

    moles H2 = 2 g / 2g/mol = 1 mole H2

    moles O2 = 32 g / 32g/mol = 1 mole O2

    2H2 + O2 - - > 2H2O

    i 1 1 0

    c 1 0.5 1

    e 0 0.5 1

    Assuming the reaction will proceed, there will be an excess of 0.5 mol O2 and a product of 1 mol H2O. This gives 18 grams of water.
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