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16 May, 15:45

Zn+2HCl⇒ZnCl₂+H₂

Assuming you start with 10.0 g of zinc and 10.0 g hydrochloric acid, identify the limiting reagent and determine what mass of the other will remain after the reaction runs to completion.

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  1. 16 May, 16:40
    0
    The balanced chemical reaction for the substances given would be as follows:

    Zn + 2HCl = ZnCl2 + H2

    We are given the amounts of the reactants used in the reaction. We use these amounts to determine which is the limiting and excess reactant. We do as follows:

    10 g Zn (1 mol / 65.38 g) = 0.1530 mol

    10 g HCl (1 mol / 36.46 g) = 0.2743 mol

    From the the stoichiometric ratio which is 1 is to 2, the limiting reactant would be hydrochloric acid and the excess would be zinc metal.

    Mass of zinc that remains = 0.1530 - (0.2743 / 2) = 0.0159 g Zn
  2. 16 May, 19:23
    0
    The equation shows that one mole of Zn requires 2 moles of HCl. We now calculate the moles of each specie:

    Zn = 10/65 = 0.154 mole

    HCl = 10/36.5 = 0.274 mole

    Molar ratio present:

    1: 1.78; thus, the HCl is the limiting reactant

    Moles of Zn reacted = 0.274/2 = 0.137

    Moles of Zn remaining = 0.154 - 0.137

    = 0.017 moles

    Mass of Zn left = 0.017 x 65

    = 1.105 grams
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