A 1.25 g sample of aluminum is reacted with 3.28 g of copper (II) sulfate. What is the limiting reactant? 2Al(s) + 3CuSO4(aq) = Al2(SO4)3(aq) + 3Cu(s)
Select one:
a)Copper
b)Aluminum sulfate
c)Aluminum
d)Copper (II) sulfate

d. Copper (II) sulfate

Explanation:

Given data:

Mass of Al = 1.25 g

Mass of CuSO₄ = 3.28 g

What is limiting reactant = ?

Solution:

Chemical equation:

2Al + 3CuSO₄   →   Al₂ (SO₄)₃ + 3Cu

Number of moles of Al:

Number of moles = mass/molar mass

Number of moles = 1.25 g/ 27 g/mol

Number of moles = 0.05 mol

Number of moles of CuSO₄:

Number of moles = mass/molar mass

Number of moles = 3.28 g/ 159.6 g/mol

Number of moles = 0.02 mol

now we will compare the moles of reactant with product.

              Al           :           Al₂ (SO₄)₃

                2          :             1

              0.05       :          1/2×0.05=0.025 mol

               Al           :            Cu

                2            :              3

              0.05         :            3/2×0.05 = 0.075 mol

        CuSO₄           :           Al₂ (SO₄)₃

               3             :             1

              0.02         :          1/3×0.02=0.007 mol

        CuSO₄           :            Cu

              3               :              3

              0.02         :              0.02  

Less number of moles of reactants are produced by CuSO₄ thus it will act as limiting reactant.

a electronegativity decreases beacuse the size of nucleus is bigger.