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 data:

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

catya your not at all which answer i've seen you do this on another question!

the objects have the same charge is correct.

nathan lee