The standard e.m.f. of the following cell is 0 . 463 V Cu s | Cu + + 1 M | | Ag + 1 M | Ag s If the standard potential of Ag electrode is 0 . 800 V , what is the standard potential of Cu electrode?

The given cell, Cu s | Cu + + 1 M | | Ag + 1 M | Ag s As we know, the standard potential of the cell is calculated by using the formula: E cell ∘ = E cathode ∘ - E anode ∘ Given, E cell ∘ = 0 . 463 V , The standard potential of silver electrode, E cathode ∘ = 0 . 8 V The standard potential of copper electrode, E anode ∘ = E cathode ∘ - E cell ∘ E anode ∘ = 0 . 8 - 0 . 463 E anode ∘ = 0 . 337 V From the above, it is clear that the standard potential of Cu electrode is 0 . 337 V .

Write the cell reaction and calculate E ° cell of the following electrochemical cell: Al s | Al 3 + aq . ( 1 M ) | | Zn 2 + aq . ( 1 M ) | Zn s E ° Al = - 1 . 66 V E ° Zn = - 0 . 76 V

The given electrochemical cell, Al s | Al 3 + aq . ( 1 M ) | | Zn 2 + aq . ( 1 M ) | Zn s As we know, the standard potential of the cell is calculated by using the formula: E cell ∘ = E cathode ∘ - E anode ∘ Given, E ° Al = - 1 . 66 V E ° Zn = - 0 . 76 V The standard potential of zinc electrode, E cathode ∘ = - 0 . 76 V The standard potential of aluminium electrode, E anode ∘ = - 1 . 66 V E Cell ∘ = - 0 . 76 - ( - 1 . 66 ) E Cell ∘ = - 0 . 76 + 1 . 66 E Cell ∘ = 0 . 9 V From the above, it is clear that the E ° Cell for the given electrochemical cell is 0 . 9 V .

Represent a cell consisting of Mg 2 + | Mg half cell and Ag + | Ag half cell and write the cell reaction. ( E ° Ag = 0 . 799 V , E ° Mg = - 2 . 37 V )

The given data shows that Mg undergoes oxidation and Ag + undergoes reduction. Hence, cell reaction is: Mg ( s ) → Mg 2 + + 2 e - ( oxidation half reaction ) 2 Ag + + 2 e - → 2 Ag ( reduction half reaction ) Mg ( s ) + 2 Ag + → Mg 2 + + 2 Ag ( overall cell reaction ) The cell representation is: Mg s | Mg aq 2 + ( x M ) | | Ag aq + ( y M ) | Ag s

How much quantity of electricity in coulomb is required to deposit 1 . 346 × 10 - 3 kg of Ag in 3 . 5 minutes from AgNO 3 solution? (Given : Molar mass of Ag is 108 × 10 - 3 kg mol - 1 )

Given: Mass of Ag deposited = 1 . 346 × 10 - 3 kg Time (t)= 3 . 5 minutes Molar mass of Ag= 108 × 10 - 3 kg mol - 1 To calculate: Quantity of electricity required in coulomb We know, mole ratio = moles of product formed in half reaction moles of electrons required in half reaction mass of the substance produced = I ( A ) × t ( s ) 96500 ( C / mol e - ) × mole ratio × molar mass of substance quantity of electricity in coulomb ( Q ) = I ( in amp ) × t ( in sec ) Calculation: The half reaction for the formation of Ag is, Ag ( aq ) + + e - → Ag ( s ) mole ratio = 1 mol Ag / mol e - 1 . 346 × 10 - 3 = I × 3 . 5 × 60 96500 × 1 × 108 × 10 - 3 I = 1 . 346 × 10 - 3 × 96500 1 × 108 × 10 - 3 × 3 . 5 × 60 = 5 . 727 A Q = It = 1202 . 67 C

Write the cell reaction and calculate E ° cell of the following electrochemical cell: Al s | Al 3 + aq . ( 1 M ) | | Zn 2 + aq . ( 1 M ) | Zn s E ° Al = - 1 . 66 V E ° Zn = - 0 . 76 V

The given electrochemical cell, Al s | Al 3 + aq . ( 1 M ) | | Zn 2 + aq . ( 1 M ) | Zn s As we know, the standard potential of the cell is calculated by using the formula: E cell ∘ = E cathode ∘ - E anode ∘ Given, E ° Al = - 1 . 66 V E ° Zn = - 0 . 76 V The standard potential of zinc electrode, E cathode ∘ = - 0 . 76 V The standard potential of aluminium electrode, E anode ∘ = - 1 . 66 V E Cell ∘ = - 0 . 76 - ( - 1 . 66 ) E Cell ∘ = - 0 . 76 + 1 . 66 E Cell ∘ = 0 . 9 V From the above, it is clear that the E ° Cell for the given electrochemical cell is 0 . 9 V .

E M B I B E

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Electrochemistry>Maharashtra Board-2018>Q 4

EASY

12th Maharashtra Board

IMPORTANT

Earn 100

The S.I. unit of cell constant for conductivity cell is :

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Important Questions on Electrochemistry

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12th Maharashtra Board

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Electrochemistry>Maharashtra Board-2019>Q 5

How many faradays of electricity are required to produce

6 g

of

Mg

from

{MgCl}_{2}

?

HARD

12th Maharashtra Board

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Electrochemistry>Maharashtra Board-2019>Q 6

The molar conductivity of

0.05 M {BaCl}_{2}

solution at

25 ° C

is

223 Ω^{- 1} {cm}^{2} {mol}^{- 1}

. What is its conductivity?

HARD

12th Maharashtra Board

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Electrochemistry>Maharashtra Board-2019>Q 7

Define electrochemical series. Write its applications.

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12th Maharashtra Board

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Electrochemistry>Maharashtra Board-2020>Q 8

The standard e.m.f. of the following cell is $0.463 V$

$\underset{(s)}{Cu} | \underset{(1 M)}{{Cu}^{+ +}} | | \underset{(1 M)}{{Ag}^{+}} | \underset{(s)}{Ag}$
If the standard potential of $Ag$ electrode is $0.800 V$ , what is the standard potential of $Cu$ electrode?

HARD

12th Maharashtra Board

IMPORTANT

EMBIBE CHAPTER WISE PREVIOUS YEAR PAPERS FOR CHEMISTRY>Chapter 4 - Electrochemistry>Maharashtra Board-2020>Q 9

Write the cell reaction and calculate $E^{°}$ cell of the following electrochemical cell:
$\underset{(s)}{Al} | \underset{(1 M)}{\underset{(aq .)}{{Al}^{3 +}}} | | \underset{(1 M)}{\underset{(aq .)}{{Zn}^{2 +}}} | \underset{(s)}{Zn}$