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Standard XII

Chemistry

Oxidizing Nature of Sulphuric Acid

Electrolysis ...

Question

Electrolysis of $H_{2} S O_{4}$ produces _______at anode.

H_{2}

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O_{2}

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H_{2} S_{2} O_{8}

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H_{2} S_{2} O_{3}

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Solution

The correct option is C $H_{2} S_{2} O_{8}$
$H_{2} S O_{4} \to 2 H^{+} + S O_{4}^{2 -}$
At anode, following reaction occurs.
$2 S O_{4}^{2 -} \to S_{2} O_{8}^{2 -} + 2 e^{-}$
After, $S_{2} O_{8}^{2 -}$ reacts with $H^{+}$ to form $H_{2} S_{2} O_{8}$

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Similar questions

Q. Marshall's acid or perdisulphuric acid

(H_{2} S_{2} O_{8})

can be prepared by electrolytic oxidation of

H_{2} S O_{4}

as :

2 H_{2} S O_{4} \to H_{2} S_{2} O_{8} + 2 H^{\oplus} + 2 e^{-}

O_{2}

and

H_{2}

are byproducts. In such an electrolysis 9.72 L of

H_{2}

and 2.35 L of

O_{2}

were produced at S.T.P. What is the weight of

H_{2} S_{2} O_{8}

formed ?

Q. During the preparation of

H_{2} S_{2} O_{8}

(per disulphuric acid)

O_{2}

gas also releases at anode as by product. When

9.72 L

H_{2}

releases at cathode and

2.35 L O_{2}

at anode at STP, the weight of

H_{2} S_{2} O_{8}

produced in gram is:

Marshalls acid is prepared by the electrolytic oxidation of $H_{2} S O_{4}$ as $2 H_{2} S O_{4} \to H_{2} S_{2} O_{8} + 2 H^{\oplus} + 2 e^{-}$

Oxygen and hydrogen are byproducts. In such Electrolysis 2.24 L of $H_{2}$ amd 0.56 L $O_{2}$ were produced at STP. The weight of $H_{2} S_{2} O_{8}$ formed is:

Q. Peroxydisulfuric acid

(H_{2} S_{2} O_{8})

can be prepared by electrolytic oxidation of

H_{2} S O_{4}

as:

2 H_{2} S O_{4} \to H_{2} S_{2} O_{8} + 2 H^{+} + 2 e

O_{2}

and

H_{2}

are by products. In such on electrolysis

0.87

g of

H_{2}

and

3.36

O_{2}

were generated at STP. Report the mass of

H_{2} S_{2} O_{8}

formed in decagram (write nearest integer).

Q. One of the methods of preparation of per disulphuric acid,

H_{2} S_{2} O_{8}

involve electrolytic oxidation of

H_{2} S O_{4}

at anode

(2 H_{2} S O_{4} \to H_{2} S_{2} O_{8} + 2 H^{+} + 2 e^{-})

with oxygen and hydrogen as by-products. In such an electrolysis,

10.08 L of H_{2}

and 2.24 L of

O_{2}

were generated at STP. What is the weight of

H_{2} S_{2} O_{8}

formed?

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Electrolysis of H2SO4 produces _______at anode.

The correct option is C H2S2O8H2SO4→2H++SO2−4At anode, following reaction occurs.2SO2−4→S2O2−8+2e−After, S2O2−8 reacts with H+ to form H2S2O8

Electrolysis of $H_{2} S O_{4}$ produces _______at anode.

The correct option is C $H_{2} S_{2} O_{8}$
$H_{2} S O_{4} \to 2 H^{+} + S O_{4}^{2 -}$
At anode, following reaction occurs.
$2 S O_{4}^{2 -} \to S_{2} O_{8}^{2 -} + 2 e^{-}$
After, $S_{2} O_{8}^{2 -}$ reacts with $H^{+}$ to form $H_{2} S_{2} O_{8}$