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28 August, 21:08

Given the balanced equation below, calculate the moles of aluminum that are needed to react completely with 17.5 moles of FeO? You must show all of your work.

2Al + 3FeO à 3Fe + Al2O3

Sodium and water react according to the following equation. If 51.5g of sodium are added to excess water, how many liters of hydrogen gas are formed at STP? Show all work for credit.

2Na + 2H2O à 2NaOH + H2

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  1. 28 August, 21:23
    0
    Question 1

    The moles off Al that are needed to react completely with 17.5 moles of FeO is 11.67 moles

    calculation

    2Al + 3 FeO→ 3 Fe + Al₂O₃

    From equation above Al: FeO is 2:3

    therefore the moles of Al = 17.5 moles x 2 / 3 = 11.67 moles

    Question 2

    The number of liters of hydrogen gas that are formed at STP 25.088 L

    calculation

    2Na + 2H₂O → NaOH + H₂

    Step 1 : calculate the moles of Na

    moles = mass: molar mass

    from the periodic table the molar mass of Na = 23 g/mol

    moles = 51.5 g: 23 g/mol = 2.24 moles

    Step 2: use the mole ratio to determine the moles of H₂

    Na:H₂ is 2:1 therefore the moles of H₂ = 2.24 moles x 1/2 = 1.12 moles

    Step 3: calculate the number of liters of H₂ at STP

    that is at STP 1 mole of a gas = 22.4 L

    1.12 moles = ? L

    by cross multiplication

    = (1.12 moles x 22.4 L) / 1 mole = 25.088 L
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