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6 January, 03:06

Using the ideal gas law and stoichiometry calculations, determine the amount of zinc metal needed to produce 150 ml of h2 gas at 293 k via the oxidation reaction below

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  1. 6 January, 05:15
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    You did not include the reaction.

    This reaction meets the statement:

    Zn + 2 HCl - - - > ZnCl2 + H2 (g)

    So, I am going to show you how to solve the problem, from that reaction.

    dа ta:

    Zn = ?

    V = 150 ml

    T = 293 k

    I also have to assume atmospheric pressure, p = 1 atm

    1) Determine the number of moles of H2 gas, using ideal gas law.

    pV = nRT = > n = pV / RT = 1 atm * 0,150 liter / (0,0821 atm*liter/K*mol * 293 k)

    => n = 0,0062 mol H2

    2) State the molar ratios from the reaction:

    1 mol Zn : 1 mol H2

    3) State the proportion with 0,0062 mol H2

    1 mol Zn / 1 mol H2 = x mol Zn / 0,0062 mol H2 = >

    x = 0,0062 mol Zn

    4) Determine the mass of Zn using the atomic mass of Zn: 65.39 g/mol

    => mass of Zn = 0,0062 mol * 65,39 g / mol = 0,41 g

    Answer: 0,41 g
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