Given below are the half - cell reactions : Mn 2 + + 2 e - → Mn ; E ∘ = - 1.18 V 2 Mn 3 + + e - → Mn 2 + ; E ∘ = + 1.51 V The E ∘ for 3 Mn 2 + → Mn + 2 Mn 3 + will be :

- 2.69 V ; the reaction will not occur

- 2.69 V ; the reaction will occur

- 0.33 V ; the reaction will not occur

- 0.33 V ; the reaction will occur

Consider the following standard electrode potentials ( E o in volts) in aqueous solution: E l e m e n t M 3 + / M M + / M A l - 1.66 + 0.55 T l + 1.26 - 0.34 Based on these data, which of the following statements is correct?

T l + is more stable than A l +

T l + is more stable than A l 3 +

A l + is more stable than A l 3 +

T l 3 + is more stable than A l 3 +

EASY

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Using the standard electrode potentials given below, predict if the reaction between the following is feasible.

Fe³⁺ (aq) and I^- (aq) & report the value of $E_{cell}^{o}$

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Important Questions on Electrochemistry

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Given

E_{{Cl}_{2} / {Cl}^{-}}^{o} = 1 .36 V, E_{{Cr}^{3 +} / Cr}^{o} = - 0 .74 V

E_{{Cr}_{2} O_{7}^{2 -} / {Cr}^{3 +}}^{o} = 1 .33 V, E_{{MnO}_{4}^{-} / {Mn}^{2 +}}^{o} = 1 .51 V .

Among the following, the strongest reducing agent is:

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

In an electrochemical cell, anode and cathode are respectively

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

In a electrochemical cell, the reaction will be feasible when

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Four successive members of the first row of transition elements are listed below with atomic numbers. Which one of them is expected to have the highest

E_{M^{3 +} / M^{2 +}}^{o}

value?

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Standard hydrogen electrode (SHE) is a

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

The standard emf of the cell

Zn ∣ {Zn}^{2 +} ‖ {Ag}^{+} | Ag

1.56 V .

If the standard reduction potential of

Ag

0.8 V,

the standard oxidation potential of

Zn

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

The standard emf of

Zn

Cu

voltaic cell is

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Consider the cell at $25 ° C$

$Zn |{Zn}^{2 +} (aq), (1 M) ‖ {Fe}^{3 +} (aq), {Fe}^{2 +} (aq)| Pt (s)$

The fraction of total iron present as ${Fe}^{3 +}$ ion at the cell potential of $1.500 V$ is $x \times 10^{- 2}$ . The value of $x$ is ______. (Nearest integer)

$Given : {E^{\circ}}_{{Fe}^{3 +} | {Fe}^{2 +}} = 0.77 V, {E^{\circ}}_{{Zn}^{2 +} | Zn} = - 0.76 V$

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Given that the standard potentials

(E^{o})

{Cu}^{2 +} / Cu

and

{Cu}^{+} / Cu

are

0.34 V

and

0.522 V

respectively, the

E^{o}

{Cu}^{2 +} / {Cu}^{+}

is:

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Identify the reaction from following having top position in electrochemical series according to their standard electrode potential.

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

What will be the oxidation potential for the following hydrogen half cell at $1$ bar pressure and $25 º C$ temperature?

$Pt |\underset{1 bar}{H_{2 (g)}}| {HCl}_{(aq)} pH = 3$

HARD

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Given below are the half - cell reactions :

\begin{matrix} {Mn}^{2 +} + 2 e^{-} \to Mn; & E^{\circ} = - 1.18 V \\ 2 ({Mn}^{3 +} + e^{-} \to {Mn}^{2 +}); & E^{\circ} = + 1.51 V \end{matrix}

The

E^{\circ}

for

3 {Mn}^{2 +} \to Mn + 2 {Mn}^{3 +}

will be :

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

In which metal container, the aqueous solution of ${CuSO}_{4}$ can be stored?

$E_{{Cu}^{3 +} / Cu}^{0} = 0.34 V$

$E_{F e / F e^{2 +}}^{0} = 0.44 V, E_{A l / A^{3 +}}^{0} = 1.66 V$

$E_{N i / N^{2 +}}^{0} = 0.25 V, E_{A g^{+} / A g}^{0} = 0.80 V$

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

A variable, the opposite external potential

(E_{ext})

is applied to the cell

Z n | Z n^{2 +} (1 M) ∥ C u^{2 +} (1 M) | C u

, of potential

1.1 V

. When

E_{e x t} < 1.1 V

and

E_{e x t} > 1.1 V

, respectively electrons flow from

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Four metals

W, X, Y

and

Z

have standard electrode potential as

- 0.13 V, - 0.85 V, - 0.25 V

and

+ 0.22 V

respectively. The most reducing metal is

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

The hydrogen ion concentration in a standard hydrogen electrode is

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

What will be the half-cell potential of a hydrogen electrode acting as an anode and dipped in a solution of

pH = 2 ?

EASY

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Given the standard half-cell potentials $(E °)$ of the following as

$Zn ⟶ {Zn}^{2 +} + 2 e^{-}; E ° = + 0.76 V$

$Fe ⟶ {Fe}^{2 +} + 2 e^{-}; E ° = + 0.41 V$

Then the standard e.m.f. of the cell with the reaction ${Fe}^{2 +} + Zn ⟶ {Zn}^{2 +} + Fe$ is

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Calculate the standard cell potential (in V) of the cell in which the following reaction takes place:

${F e}^{2 +} (a q) + A g^{+} (a q) \to F e^{3 +} (a q) + A g (s)$

Given that
$E_{{Ag}^{+} / A g}^{o} = x V$
$E_{{F e}^{2 +} / F e}^{o} = y V$
$E_{{F e}^{3 +} / F e}^{o} = z V$

MEDIUM

Chemistry>Physical Chemistry>Electrochemistry>Electrode Potential and Standard Electrode Potential

Consider the following standard electrode potentials (

E^{o}

in volts) in aqueous solution:

\begin{matrix} \underset{}{E l e m e n t} & \underset{}{M^{3 +} / M} & \underset{}{M^{+} / M} \\ A l & - 1.66 & + 0.55 \\ T l & + 1.26 & - 0.34 \end{matrix}

Based on these data, which of the following statements is correct?

Using the standard electrode potentials given below, predict if the reaction between the following is feasible. Fe3+ (aq) and I- (aq) & report the value of E cell o

Important Questions on Electrochemistry

Learn and Prepare for any exam you want !

Using the standard electrode potentials given below, predict if the reaction between the following is feasible.

Fe³⁺ (aq) and I^- (aq) & report the value of $E_{cell}^{o}$