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26 June, 13:53

Molten gallium reacts with arsenic to form the semiconductor, gallium arsenide, GaAsGaAs, used in light emitting diodes and solar cells: Ga (l) + As (s) → GaAs (s) Ga (l) + As (s) → GaAs (s) If 4.00 gg of gallium is reacted with 5.50 gg of arsenic how many grams of the excess reactant are left at the end of the reaction?

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  1. 26 June, 17:43
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    1.195 g of Arsenic.

    Explanation:

    Equation of the reaction:

    Ga (l) + As (s) → GaAs (s).

    Calculating the limiting reagent by:

    Number of moles of:

    Gallium:

    Molar mass of Gallium = 69.7 g/mol.

    Mass = 4 g

    Number of moles = mass/molar mass

    = 4/69.7

    = 0.0574 mol.

    Arsenic:

    Molar mass of Arsenic = 75 g/mol.

    Mass = 5.5 g

    Number of moles = mass/molar mass

    = 5.5/75

    = 0.0733 mol

    Therefore, using stoichiometry since 1 mole of Gallium reacted with 1 mole of Arsenic. The limiting reagent is Gallium.

    Excess reagent is Arsenic.

    Number of moles excess = 0.0733 - 0.0574

    = 0.0159 moles

    Mass of the excess Arsenic left =

    Molar Mass * number of moles

    = 0.0159 * 75

    = 1.195 g of Arsenic.
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