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Standard XII

Chemistry

Chemical Properties of Ethers

Peroxydisulfu...

Question

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 $3.36$ g $O_{2}$ were generated at STP. Report the mass of $H_{2} S_{2} O_{8}$ formed in decagram (write nearest integer).

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Solution

$2 H_{2} S O_{4} ⟶ H_{2} S O_{8} + 2 H^{+} + 2 e$
$n_{H_{2}} = \frac{0.87}{2} = 0.435$
$n_{O_{2}} = 0.105$
$n_{H_{2} S O_{8}} = 1 - (0.435 + 0.105) 0.46$
$m = 0.46 \times 98 = 45.08 g$
$m = 4$ decagram

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Similar questions

Q. Peroxy disulphuric 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^{-}

Oxygen and hydrogen are by products. In such an electrolysis

9.72 l i t r e

H_{2}

and

2.35

litre of

O_{2}

were generated at NTP. What is the mass of peroxy disulphuric acid formed?

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. 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 node

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

with oxygen and hydrogen as by -products. In such an electrolysis, 9.722 L of

H_{2}

and 2.35 L of

O_{2}

were generated at STP. What is the weight of

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

formed in gms? (write the value to the nearest integer).

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. 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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Peroxydisulfuric acid (H2S2O8) can be prepared by electrolytic oxidation of H2SO4 as:2H2SO4→H2S2O8+2H++2e. O2 and H2 are by products. In such on electrolysis 0.87 g of H2 and 3.36 g O2 were generated at STP. Report the mass of H2S2O8 formed in decagram (write nearest integer).

2H2SO4⟶H2SO8+2H++2enH2=0.872=0.435nO2=0.105nH2SO8=1−(0.435+0.105)0.46m=0.46×98=45.08 gm=4 decagram

$2 H_{2} S O_{4} ⟶ H_{2} S O_{8} + 2 H^{+} + 2 e$
$n_{H_{2}} = \frac{0.87}{2} = 0.435$
$n_{O_{2}} = 0.105$
$n_{H_{2} S O_{8}} = 1 - (0.435 + 0.105) 0.46$
$m = 0.46 \times 98 = 45.08 g$
$m = 4$ decagram