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 +

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

HARD

Earn 100

The standard potential of the following cell is 0.23 V at $15 ° C$ and 0.21 V at $35 ° C$ .

$Pt (s) | H_{2} (g) | HCl (aq) | AgCl (s) | Ag (s)$

(ii) Calculate $Δ H ° a n d Δ S °$ for the cell reaction by assuming that these quantities remain unchanged in the range $15 ° C to 35 ° C$ .

(iii) Calculate the solubility of AgCl in water at $25 ° C$ .

Given: The standard reduction potential of the ${Ag}^{+} (aq) / Ag (s)$ couple is 0.80 V at $25 ° C$ .

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Important Questions on Electrochemistry

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

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

EASY

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

In an electrochemical cell, anode and cathode are respectively

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?

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

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

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

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

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 ?

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

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

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:

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?

MEDIUM

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

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

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

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

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

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 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

Consider the following electrodes

$P = {Zn}^{2 +} (0.0001 M) / Zn Q = {Zn}^{2 +} (0.1 M) / Zn$

$R = {Zn}^{2 +} (0.01 M) / Zn S = {Zn}^{2 +} (0.001 M) / Zn$

$E_{{Zn}^{2 +} / Zn}^{o} = - 0.76 V$ electrode potentials of the above electrodes in volts are in the order

EASY

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

The hydrogen ion concentration in a standard hydrogen electrode is

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:

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

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

Important Questions on Electrochemistry

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