Given: C o 3 + + e - → C o 2 + ; E ° = + 1.81 V P b 4 + + 2 e - → P b 2 + ; E ° = + 1.67 V C e 4 + + e - → C e 3 + ; E ° = + 1.61 V B i 3 + + 3 e - → B i ; E ° = + 0.20 V Oxidizing power of the species will increase in the order:

B i 3 + < C e 4 + < P b 4 + < C o 3 +

C o 3 + < C e 4 + < B i 3 + < P b 4 +

C o 3 + < P b 4 + < C e 3 + < B i 3 +

C e 4 + < P b 4 + < B i 3 + < C o 3 +

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Standard electrode potential of three metals A, B and C are $+ 0. 5 V,$ $- 3 .0 V and - 1 . 2 V$ respectively. The reducing power of these metals are

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Important Questions on Electrochemistry

EASY

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

What is an electrochemical series? How is it useful in predicting whether a metal can liberate hydrogen from acid or not?

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

Consider the following reduction processes:

{Zn}^{2 +} + 2 e^{-} \to Zn (s); E^{o} = - 0 .76 V

{Ca}^{2 +} + 2 e^{-} \to Ca (s); E^{o} = - 2 .87 V

{Mg}^{2 +} + 2 e^{-} \to Mg (s); E^{o} = - 2 .36 V

{Ni}^{2 +} + 2 e^{-} \to Ni (s); E^{o} = - 0 .25 V

The reducing power of the metals increases in the order:

EASY

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

For the cell $Cu (s) |{Cu}^{2 +} (aq) (0.1 M) ‖ {Ag}^{+} (aq) (0.01 M)| Ag (s)$ the cell potential $E_{1} = 0.3095 V$ . For the cell $Cu (s) |{Cu}^{2 +} (aq) (0.01 M) ‖ {Ag}^{+} (aq) (0.001 M)| Ag (s)$ the cell potential $= x \times 10^{- 2} V .$ Find value of x (Round off the Nearest Integer).

[ Use $: \frac{2.303 RT}{F} = 0.059 J$ ]

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

Given

E_{{Cr}^{3 +} / Cr}^{o} = - 0.74 {V;  E}_{{MnO}_{4}^{-} / {Mn}^{2 +}}^{o} = 1.51 V

E_{{Cr}_{2} O_{7}^{2 -} / {Cr}^{3 +}}^{o} = 1.33 {V;   E}_{{Cl}_{2} | {Cl}^{-}}^{o} = 1.36 V

Based on the data given above, strongest oxidising agent will be:

EASY

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

The standard electrode potentials

(E_{M^{+} / M}^{o})

of four metals

A, B, C

and

D

are

- 1 .2 V,

0 .6 V

0 .85 V

and

- 0 .76 V

, respectively. The sequence of deposition of metals on applying potential is

HARD

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

What is electrochemical series? Describe kohlrausch's law and give its two applications.

EASY

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

In which of the following cases a chemical reaction is possible?

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

What is Electrochemical series? Mention its important applications.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

Given that,

$E_{O_{2} / H_{2} O}^{o} = + 1 .23 V;$
$E_{S_{2} O_{8}^{2 -} / {SO}_{4}^{2 -}}^{o} = 2 .05 V$
$E_{{Br}_{2} / {Br}^{-}}^{o} = + 1.09 V;$
$E_{{Au}^{3 +} / Au}^{o} = 1 .4 V$

The strongest oxidizing agent is

HARD

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

Given:

C o^{3 +} + e^{-} \to C o^{2 +}; E ° = + 1.81 V

{P b}^{4 +} + {2 e}^{-} \to {P b}^{2 +}; E ° = + 1.67 V

C e^{4 +} + e^{-} \to C e^{3 +}; E ° = + 1.61 V

{B i}^{3 +} + {3 e}^{-} \to B i; E ° = + 0.20 V

Oxidizing power of the species will increase in the order:

HARD

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

Define electrochemical series. Write its applications.

EASY

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

The standard reduction potentials (in V) of a few metal ion/metal electrodes are given below.

{Cr}^{3 +} / Cr = - 0 .74; {Cu}^{2 +} / Cu = + 0 .34; {Pb}^{2 +} / Pb = - 0 .13; {Ag}^{+} / Ag = + 0 .8 .

The reducing strength of the metals follows the order

EASY

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

The position of some metals in the electrochemical series in decreasing electropositive character is

Mg > Al >

Zn > Cu > Ag .

The change expected on stirring the solution of aluminium nitrate with copper spoon is

EASY

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

Define the term:

Electrochemical series

EASY

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

Following four colourless solutions of salts have been kept in different test tubes and a copper strip was dipped in each. Which solution will turn blue in the end?

HARD

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

The standard electrode potential of

M^{2 +} / M

is positive for

HARD

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

Two identical beakers contain concentrated $HCl$ solution at $298 K$ . In the first beaker solid $Cu$ is added, while in the second beaker solid $Zn$ is added. Which of the following will be observed?

$[E^{0} ({Zn}^{2 +} / Zn) = - 0.76 V; E^{0} ({Cu}^{2 +} / Cu) = + 0.34 V]$

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

250 mL

of a waste solution obtained from the workshop of a goldsmith contains

0.1 M {AgNO}_{3}

and

0.1 M AuCl

. The solution was electrolyzed at

2 V

by passing a current of

1 A

for

15

minutes. The metal/metals electrodeposited will be :

(E_{{Ag}^{+} / Ag}^{0} = 0.80 V, E_{{Au}^{+} / Au}^{0} = 1.69 V)

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

The metal that cannot be obtained by the electrolysis of an aqueous solution of its salt is

EASY

Chemistry>Physical Chemistry>Electrochemistry>Nernst Equation

Which of the following ions does not liberate hydrogen gas on reaction with dilute acids?

Standard electrode potential of three metals A, B and C are + 0.5 V, –3.0 V and –1.2 V respectively. The reducing power of these metals are

Important Questions on Electrochemistry

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Standard electrode potential of three metals A, B and C are $+ 0. 5 V,$ $- 3 .0 V and - 1 . 2 V$ respectively. The reducing power of these metals are