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Catalyst-Positive,Negative, Biological

5.5g of a mix...

Question

5.5g of a mixture of FeSO4.7H2O and Fe2(SO4)3.9H2O requires 5.4ml of 0.1N KMnO4 solution for complete oxidation.calculate the number of gram mole of hydrated ferric sulphate in the mixture.

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F e S O_{4} . 7 H_{2} O

F e_{2} (S O_{4})_{3} .

9 H_{2} O

K M n O_{4}

5.5

F e S O_{4} .7 H_{2} O

F e_{2} (S O_{4})_{3} .9 H_{2} O

5.4

0.1 N K M n O_{4}

9.52 \times 10^{- x}

x

5.5

F e S O_{4} .7 H_{2} O

F e_{2} (S O_{4})_{3} .9 H_{2} O

5.4

0.1

N

K M n O_{4}

N O_{2}

N_{2} O_{4}

38.3

{26.7}^{o} C

N O_{2}

100

5.5 g

F e S O_{4} \cdot 7 H_{2} O

F e_{2} (S O_{4})_{3} \cdot 9 H_{2} O

5.4 m L

0.1 N K M n O_{4}

H = 1, O = 16, S = 32, F e = 56

1 mole of equimolar mixture of ferric oxalate and ferrous oxalate will require x mole of $K M n O_{4}$ in acidic medium for complete oxidation, x is

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