notes 1 electrolytic cell

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It is the detailed study of relation between current electricity and chemical reaction

electrochemistry

That device in which chemical reaction occur when current is passed through certain solution

electrolytic cell

That device in which current in generated due to occurrence of certain reaction

galvanic cell

Electrolytic and galvanic cell combined called as

electrochemical cell

In electrochemical cell reduction occurs at which electrode

cathode

In electrochemical cell oxidation occurs at which electrode

anode

In electrolysis of aqueous NaCl solution products obtained at anode and cathode respectively

Cl2. H2

Cations having more reduction potential gets reduced at which electrode. In preferential discharge theory

cathode

Anions having more oxidation potential gets oxidise at which electrode. In preferential discharge theory

anode

More is the reduction potential of an element more is the tendency to get

reduced

If aqueous solution of sulphuric acid is electrolysed using platinum electrodes than products at cathode and anode respectively are

hydrogen and Oxygen gas

If aqueous solution of copper sulphate is electrolysed using platinum electrodes then product obtained at cathode and anode respectively are

If aqueous solution of NaCl is electrolysed using Hg or calomel electrode than product obtained at cathode and anode respectively are

If aqueous solution of copper sulphate is electrolysed using copper electrodes than product obtained at anode and cathode respectively are

Reduction and oxidation potential also depend upon concentration of ions

If electrolysis of concentrated copper sulphate solution is done using platinum electrodes then products obtained at cathode and anode respectively are

Calculate the product at cathode and anode if aqueous solution ofsodium sulphate is electrolysed using Mercury electrode

Na-Hg & O2

Calculate the product obtands at cathode and anode it concentrated sulphuric acid solution is electrolyzed using platinum electrode

Products at cathode and anode if Aqueous zinc sulphate solution is electrolysed using platinum electrode

Zn. O2

State faraday's first law of electrolysis

Mass of element deposited by 1 coulomb charge is known as

electrochemical equivalent

Total charge on one mole electrons in coulomb equal to

96500C

Calculate the charge required to deposit 9 gram. Al³+ ion

1 F

The current in a given wire is 1.8A . the number of coulombs that flow in 1.36 minute will be

147C

0.1cm

How much current must be passed through aqueous NaCl solution for 100 second in order to prepare 23 gram of 20% by mass Na-Hg amalgam using Hg electrodes

193C

Two electrolytic cells /voltameter are connected in a series and a current is passed for 10 second if 6 gram of aluminium ion and deposited then what weight of Zn will be deposited in same time

21.6gm

Solute solute interaction is also known as

asymmetry effect

In electrolysis Solvent solute interaction is also known as

electrophoretic effect

In electrolytic conductance due to solute solute interaction and solvent solute interaction conductance increases or decreases respectively

increases & increases

On increasing temperature electrolytic resistance decreases or increases

decreases

On dilution specific conductivity of a solution decreases or increases

decreases

Calculate specific conductivity of 0.1 M KCl solution which is present in a cell of length 2 cm and area cross section 10 cm² .resistance of this solution is found to be 100 ohm

0.002 Scm-¹

Specific conductivity of a 0.1M NaCl solution is found to be 0.01 Scm-¹ and resistance of this solution is 100 ohm calculate specific conductivity of 0.01M KCl solution taken in same electrolyte cell if its resistance is found to be 50 ohm

0.02 Scm-¹

Calculate the resistance of NaCl solution which specific conductivity is 10 Sm-¹ and cell constant is found to be 1cm-¹

10ohm

2.5 F of electricity are passed through a copper sulphate solution the number of gram equivalent of copper deposited on cathode is

2.5

Calculate molar conductivity of 0.1 M KCl solution whose specific conductivity is 10 Sm-¹

1000 Scm²mol-¹

Calculate the molar conductivity of 0.01 M NaCl solution which has resistance of 100 ohm and cell constant is 10 m-¹

10-² Scm²mol-¹

Specific conductance of 0.1 M nitric acid is 0.063 Scm-¹ the molar conductance of the solution is

630 Scm²mol-¹

On dilution in strong electrolytes molar conductivity of strong electrolytes increases

Debye huckel onsanger theory is for

strong electrolytes only

On dilution molar conductivity of weak electrolyte

increases

Molar conductivity at infinite dilution for weak electrolytes can be determined by extrapolating curve on debye huckel onsanger graph

Kohlrausch law states that

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