Question

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​

Answer 1

55.1 g NiCl2

Step-by-step explanation:

According to a study done in 1683, that is the answer.

Answer 2

55.73 g

Step-by-step 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