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

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Among the following reduction processes, what is correct increasing order of reducing power of the metals?

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

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

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

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

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Important Questions on Redox Reactions and Electrochemistry

EASY

Chemistry>Physical Chemistry>Redox Reactions and 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

HARD

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

The standard reduction potential for ${Cu}^{2 +} / Cu$ is $+ 0.34 V .$ Calculate the reduction potential at $pH =14$ for the above couple.

$(K_{sp} of Cu {(OH)}_{2} = 1 \times 10^{- 19})$

MEDIUM

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

In a electrochemical cell, the reaction will be feasible when

MEDIUM

Chemistry>Physical Chemistry>Redox Reactions and 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?

EASY

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

The standard emf of

Zn

Cu

voltaic cell is

MEDIUM

Chemistry>Physical Chemistry>Redox Reactions and 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>Redox Reactions and 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

HARD

Chemistry>Physical Chemistry>Redox Reactions and 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>Redox Reactions and 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>Redox Reactions and 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

MEDIUM

Chemistry>Physical Chemistry>Redox Reactions and 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?

MEDIUM

Chemistry>Physical Chemistry>Redox Reactions and 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?

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

EASY

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

In an electrochemical cell, anode and cathode are respectively

MEDIUM

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

The hydrogen ion concentration in a standard hydrogen electrode is

EASY

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

Standard hydrogen electrode (SHE) is a

MEDIUM

Chemistry>Physical Chemistry>Redox Reactions and 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

HARD

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

Consider the change in oxidation state of Bromine corresponding to different emf values, as shown in the diagram below:
Question Image

Then, what is the species undergoing disproportionation?

Among the following reduction processes, what is correct increasing order of reducing power of the metals? Zn2++2e-→Zn(s); Eo=-0.76 V Ca2++2e-→Ca(s); Eo=-2.87 V Mg2++2e-→Mg(s); Eo=-2.36 V Ni2++2e-→Ni(s); Eo=-0.25 V

Important Questions on Redox Reactions and Electrochemistry

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