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Numerical Electrolysis

The document presents a series of problems related to the quantitative aspects of electrolysis, including calculations of charge required for reductions and oxidations, coulombs needed for specific reactions, and mass of metals deposited under various conditions. It also includes questions on the electrolysis of solutions and the determination of current needed for specific rates of gas production. The problems cover a range of topics including Faraday's laws, atomic masses, and current-time relationships in electrolysis.

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Soumya Handu
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96 views2 pages

Numerical Electrolysis

The document presents a series of problems related to the quantitative aspects of electrolysis, including calculations of charge required for reductions and oxidations, coulombs needed for specific reactions, and mass of metals deposited under various conditions. It also includes questions on the electrolysis of solutions and the determination of current needed for specific rates of gas production. The problems cover a range of topics including Faraday's laws, atomic masses, and current-time relationships in electrolysis.

Uploaded by

Soumya Handu
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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Download as PDF, TXT or read online on Scribd
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PROBLEMS BASE ON:

QUANTITATIVE ASPECT OF ELECTROLYSIS


1. How much charge is required for the following reduction?

(i) 1 mol of Al3+ to Al.

(ii) 1 mol of Cu2+ to Cu.

(iii) 1 mol of MnO 4 to Mn2+

2. How many coulombs are required for the following oxidation?

(i) 1 mol of H2O to O2.

(ii) 1 mol of FeO to Fe2O3.

3. How many coulombs of electricity are required for.

(i) Complete oxidation of 90g of H2O.

(ii) Complete reduction of 100 mL of 0.1 M KMnO4 solution.

4. How much copper will be deposited on the cathode of an electrolytic cell containing copper

sulphate solution by the passage of a current of 2 amperes for 30 minutes? (At. Mass of Cu

= 63.5)

5. Two electrolytic cell containing silver nitrate solution and copper sulphate solution are

connected in series. A steady current of 2.5 ampere was passed through them till 1.078 g of

Ag were deposited. How long did the current flow? What weight of copper will be

deposited? (At. Mass of Ag = 107.8, Cu = 63.5)

6. Silver is electro-deposited on a metallic vessel of surface area 800 cm2 by passing a current

0.2 ampere for hours. Calculated the thickness of silver deposited. Give the density of silver

as 10.47 g/cc (Atomic mass of Ag = 107.92 amu)

7. In the electrolysis of acidulated water, it is desired to obtain hydrogen at the rate of 1 cc per

second at NTP condition. What should be the current passed?

8. Find the charge in coulombs on 1 g- ion of N3––

9. Calculate the number of coulombs required to deposit 40.5 g of Al when the electrode

reaction is:

Al3+ + 3e–– → Al
10. How many grams of chlorine can be produced by the electrolysis of molten NaCl with a

current of 1.00 A for 15 min?

11. How many Faradays/coulombs are required to produce.

(i) 20.0 g of calcium from molten CaCl2?

(ii) 50.0 g of aluminium from molten Al2O3.

12. Calculate the number of coulombs required is desposit 6.75 g of Al when electrode reaction

is:Al3+ + 3e–– → Al

(Given: Atomic mass Al = 27 g mol––1) F = 96500 C mol––1)

13. How many hours does it take to reduce 3 mol of Fe3+ to Fe2+ with 2.00 A current? (1 Faraday

= 96,500 C mol––1, R = 8.314 JK––1 mol––1).

14. A solution of CuSO4 is electrolyzed for 10 munities with a current of 1.5 amperes. What is

the mass of copper deposited at the cathode? (Molar mass of Cu = 63.5 g mol––1) .

15. Silver is electrodeposited on a metallic vessel of total surface area 900 cm2 by using a

current of 0.5 amp for two hours. Calculate the thickness of silver deposited. Density of

silver = 10.5 g cm-3 (Atomic mass of silver = 180 amu, F = 96500 C mol-1).

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