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9 September, 15:36

If 47.2 g of calcium chloride reacts with 135.2 g of nickel arsenate according to the following balanced equation, how many grams of nickel chloride are produced?

3CaCl2 + Ni3 (AsO4) 2--->

3NiCl2 + Can (AsO4) 2

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Answers (1)
  1. 9 September, 15:43
    0
    55.73 g

    Explanation:

    Given dа ta:

    Mass of calcium chloride = 47.2 g

    Mass of nickel arsenate = 135.2 g

    Mass of nickel chloride produced = ?

    Solution:

    Chemical equation:

    3CaCl₂ + Ni₃ (AsO₄) ₂ → 3NiCl₂ + Ca₃ (AsO₄) ₂

    Number of moles of CaCl₂:

    Number of moles = mass / molar mass

    Number of moles = 47.2 g / 110.98 g/mol

    Number of moles = 0.43 mol

    Number of moles of Ni₃ (AsO₄) ₂:

    Number of moles = mass / molar mass

    Number of moles = 135.2 g / 453.92 g/mol

    Number of moles = 0.3 mol

    Now we will compare the moles of nickel chloride with both reactant from balance chemical equation:

    CaCl₂ : NiCl₂

    3 : 3

    0.43 : 0.43

    Ni₃ (AsO₄) ₂ : NiCl₂

    1 : 3

    0.3 : 3*0.3 = 0.9

    Number of moles of NiCl₂ produced by calcium chloride are less so CaCl₂ is limiting reactant.

    Mass of NiCl₂:

    Mass = number of moles * molar mass

    Mass = 0.43 mol * 129.6 g/mol

    Mass = 55.73 g
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