Given that I 2 + 2 e - → 2 I ⊖ ; E ⊖ = 0.54 V B r 2 + 2 e - → 2 B r ⊖ ; E ⊖ = 1.69 V Predict which of the following is true

I ⊖ ions will be able to reduce bromine

B r ⊖ ions will be able to reduce iodine

Iodine will be able to reduce bromine

Bromine will be able to reduce iodide ions

Given that I 2 + 2 e - → 2 I ⊖ ; E ⊖ = 0.54 V B r 2 + 2 e - → 2 B r ⊖ ; E ⊖ = 1.69 V Predict which of the following is true

I ⊖ ions will be able to reduce bromine

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

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Given that

$I_{2} + 2 e^{-} \to 2 I^{⊖}; E^{⊖} = 0.54$ V
$B r_{2} + 2 e^{-} \to 2 B r^{⊖}; E^{⊖} = 1.69$ V

Predict which of the following is true

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Important Questions on Redox Reactions and Electrochemistry

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

In an electrochemical cell, anode and cathode are respectively

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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?

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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

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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

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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

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In a electrochemical cell, the reaction will be feasible when

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

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

pH = 2 ?

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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

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Standard hydrogen electrode (SHE) is a

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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>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?

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 standard emf of

Zn

Cu

voltaic cell is

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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

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Chemistry>Physical Chemistry>Redox Reactions and 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

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

The hydrogen ion concentration in a standard hydrogen electrode 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:

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 :

EASY

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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:

Given that I2+2e-→2I⊖;E⊖=0.54 V Br2+2e-→2Br⊖;E⊖=1.69 V Predict which of the following is true

Important Questions on Redox Reactions and Electrochemistry

Learn and Prepare for any exam you want !

Given that

$I_{2} + 2 e^{-} \to 2 I^{⊖}; E^{⊖} = 0.54$ V
$B r_{2} + 2 e^{-} \to 2 B r^{⊖}; E^{⊖} = 1.69$ V

Predict which of the following is true