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17 October, 06:34

Calculate the amount of zinc metal needed to produce 150ml of hydrogen gas at atmospheric pressure and 293 kelvin via oxidation reaction

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  1. 17 October, 07:08
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    The reaction between zinc and hydrogen gas is:

    Zn + H₂ → ZnH₂

    So for every 1 mole of H₂ gas, it needs 1 mole of Zinc. The atomic weight of H2₂ is 2 g/mol, and Zinc is 67.425 g/mol. The density of H₂ at atmospheric pressure and at 293 K is 0.00016 g/mL. The solution is as follows:

    Mass = Density*Volume = (0.00016 g/mL) (150 mL) = 0.024 g H₂

    Moles H₂ = 0.024 g H₂ * 1 mol/2 g = 0.012 mol H₂

    Thus, it also needs 0.012 mol Zn.

    Mass of Zn needed = 0.012 mol * 67.425 g/mol = 0.8091 g Zn
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