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pochemuha
3 years ago
14

An unknown metal sulfate is found to be 72.07% SO4 2- by mass. Assuming that the charge on the metal cation is +3, determine the

identity of the cation.
Chemistry
1 answer:
wariber [46]3 years ago
8 0
Lets name the unknown metal as M. Cation would be M³⁺.
the molecular formula of the compound is M₂(SO₄)₃
the mass of one mole - (molar mass of M x2 + 3 x molar mass of SO₄²⁻)
                                   = 2M + 96 x 3
                                   = 2M + 288
In 1 mol if there's 72.07% of sulphate , 
then 72.07 % corresponds to 288 g
               1 % is then      - 288/72.07 
       100 %  of the compound - 288/72.07 x 100 
 molar mass of the compound - 399.6 g/mol
mass of 2M - 399.6 - 288 = 111.6 g
molar mass of M - 111.6 /2 = 55.8 g/mol
the element with molar mass of 55.8 is Fe.
Unknown metal is iron(III) , Fe³⁺

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svetoff [14.1K]

Answer:

The answer to your question is a) 51.07 g of NiBr₂   b) Nickel, 54 g

Explanation:

Data

mass of NiBr₂ = ?

mass if Ni = 67.8 g

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Balanced chemical reaction

                Ni  +  Br₂   ⇒   NiBr₂

Process

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                    159.8 g of Br₂ --------------- 218.8 g of NiBr₂

                      37.3 g of Br₂ --------------  x

                          x = (37.3 x 218.8) / 159.8

                          x = 8161.24/159.8

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4.- Find the excess reactant

The excess reactant is Nickel

                59 g of Ni ---------------- 159.8 g of Br₂

                  x               ----------------  37.3 g of Br₂

                            x = (37.3 x 59)/159.8

                            x = 2200.7/159.8

                            x = 13.77 g of Ni

Excess Ni = 67.8 - 13.77

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