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

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