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21 January, 20:09

What mass of water can be obtained from 4.0 g of H2 and 16 g of O2?2 H2 + O2 - --> 2 H2O9 g18 g54 g36 g

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  1. 21 January, 20:16
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    There will be produced 18.02 grams of H2O

    Explanation:

    Step 1: Data given

    Mass of H2 = 4.0 grams

    Mass of O2 = 16 grams

    Molar mass of O2 = 32 g/mol

    Molar mass of H2 = 2.02 g/mol

    Molar mass of H2O = 18.02 g/mol

    Step 2: The balanced equation

    O2 + 2H2 → 2H2O

    Step 3: Calculate moles of O2

    Moles O2 = mass O2 / molar mass O2

    Moles O2 = 16.0 grams / 32. g/mol

    Moles O2 = 0.500 moles

    Step 4: Calculate moles H2

    Moles H2 = 4.0 grams / 2.02 g/mol

    Moles H2 = 1.98 moles

    Step 5: Calculate limting reactant

    For 1 mol of O2 we need 2 moles of H2 to produce 2 moles of H2O

    O2 is the limiting reactant. It will completely be consumed. (0.500 moles).

    H2 is in excess. There will be react 2*0.500 = 1.00 moles

    There will remain 1.98 - 1.00 = 0.98 moles

    Step 6: Calculate moles of H2O

    For 1 moles of O2 we need 2 moles of H2O

    For 0.500 moles of O2 consumed, we'll produce 2*0.500 = 1.00 moles of H2O

    Step 7: Calculate mass of H2O

    Mass H2O = moles H2O * molar mass H2O

    Mass H2O = 1.00 moles * 18.02 g/mol

    Mass H2O = 18.02 grams

    There will be produced 18.02 grams of H2O
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