The reaction of potassium permanganate with acidified iron [II] sulphate is given below :- $2 K M n O_{4} + 10 F e S O_{4} + 8 H_{2} S O_{4} \to K_{2} S O_{4} + 2 M n S O_{4} + 5 F e_{2} (S O_{4})_{3} + 8 H_{2} O$
If $15.8$ g of potassium permanganate was used in the reaction, calculate the mass of iron [II] sulphate used in the above reaction.
[Molecular Weight of $K = 39, M n = 55, F e = 56, S = 32, O = 16$ g/mole]

76

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152

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38

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46

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Solution

The correct option is A $76$ g
Molecular weight of $K M n O_{4} = 39 + 55 + 164 = 158$
Molecular weight of $K_{2} S O_{4} = 239 + 32 + 164 = 174$
Molecular weight of $F e S O_{4} = 56 + 32 + 164 = 152$
$2 \times$ $158$ g of $K M n O_{4}$ yields $174$ g of $K_{2} S O_{4}$
$15.8$ g of $K M n O_{4}$ will yield [( $174$ )/( $2$ $\times$ $158$ )] $\times$ $15.8$ g = $8.7$ g of $K_{2} S O_{4}$ .
$174$ g of $K_{2} S O_{4}$ yields $1520$ g of $F e S O_{4}$
$8.7$ g of $K_{2} S O_{4}$ will yield ( $1520 / 174$ ) $\times$ $8.7$ = $76$ g of $F e S O_{4}$ .
Hence, $76$ g of Iron (II) sulphate is used .

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Similar questions

The reaction of potassium permanganate (VII) with acidified iron(II) sulphate is given below:

If 15.8 g of potassium permanganate(VII) was used in the reaction, calculate the mass of iron (II) sulphate used in the above reaction. (K = 39, Mn = 55, Fe = 56, S = 32, O = 16)

(a) A flask contains 3.2 g of sulphur dioxide. Calculate the following:
(i) The moles of sulphur dioxide present in the flask.
(ii) The number of molecules of sulphur dioxide present in the flask.
(iii) The volume occupied by 3.2 g of sulphur dioxide at STP. (S = 32, O = 16)

(b) The reaction of potassium permanganate (VII) with acidified iron (II) sulphate is given below:
2KMnO₄ + 10FeSO₄ + 8H₂SO₄ $\overset{}{\to}$ K₂SO₄ + 2MnSO₄ + 5Fe₂(SO₄)₃ + 8H₂O
If 15.8 g of potassium permanganate (VII) was used in the reaction, calculate the mass of iron (II) sulphate used in the above reaction. (K = 39, Mn = 55, Fe = 56, S = 32, O = 16)

Q. Approximately how many moles of potassium permanganate,

K M n O_{4}

, are present in

40 g

of this compound? (Atomic weights:

K = 39; M n = 55; O = 16

)

Q. The reaction, is an example of reaction of:

2 M n S O_{4} + 2 K M n O_{4} + 8 H_{2} S O_{4} \to 2 M n S O_{4} + 5 F e_{2} (S O_{4})_{3} + K_{2} S O_{4} + 8 H_{2} O

When heated, potassium permanganate decomposes according to the following equation:
2KMnO₄ $\overset{}{\to}$ K₂MnO₄ + MnO₂ + O₂
(a) Some potassium permanganate was heated in a test tube. After collecting one litre of oxygen at room temperature, it was found that the test tube had undergone a loss in mass of 1.32 g. If one litre of hydrogen under the same conditions of temperature and pressure has a mass of 0.0825 g, calculate the relative molecular mass of oxygen.
(b) Given that the molecular mass of potassium permanganate is 158 g, what volume of oxygen (measured at room temperature) would be obtained by the complete decomposition of 15.8 g of potassium permanganate? (Molar volume at room temperature is 24 litres). (K = 39, Mn = 55, O = 16)

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