On the basis of standard electrode potential values, suggest which of the following reactions would take place? E Cu 2 + | Cu o = 0.34 V, E Zn 2 + | Zn o = - 0.76 V, E Mg 2 + | Mg o = - 2.37 V, E Fe 2 + | Fe o = - 0.74 V, E Br 2 | Br - o = + 1.08 V, E Cl 2 | Cl - o = + 1.36 V E Cd 2 + | Cd o = - 0.44 V (i) Cu + Zn + 2 → Cu 2 + + Zn (ii) Mg + Fe 2 + → Mg 2 + + Fe (iii) Br 2 + 2 Cl - → Cl 2 + 2 Br - (iv) Fe + Cd 2 + → Cd + Fe 2 +

(i) (ii) (iii) (iv) No Yes No Yes

(i) (ii) (iii) (iv) Yes No Yes No

(i) (ii) (iii) (iv) Yes Yes Yes No

(i) (ii) (iii) (iv) No Yes Yes Yes

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An iron wire is immersed in a solution containing ${ZnSO}_{4}$ and ${NiSO}_{4}$ . When the concentration of each salt is $1 M$ , predict which of the following reaction is likely to proceed.
Given $E^{o} ({Zn}^{+ 2} / Zn) = - 0.76 V$
$E^{o} ({Fe}^{+ 2} / Fe) = - 0.44 V$
and $E^{o} ({Ni}^{+ 2} / Ni) = - 0.25 V$

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Important Questions on Redox Reactions

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Among the following, which is the strongest oxidizing agent?

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The amount of

A g

(atomic mass = 108) deposited at the cathode when a current of 0.5 amp is passed through a solution of

A g N O_{3}

for 1 hour is closest to

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Hypophosphorus acid is a good reducing agent because

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An aqueous solution of nickel (II) sulphate was electrolyzed using nickel electrodes. Observe the diagram and answer the question that follows:

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What do you observe at the cathode and anode respectively?

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Which of the following metals will precipitate copper from copper sulphate solution?

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An aqueous solution of nickel (II) sulphate was electrolyzed using nickel electrodes. Observe the diagram and answer the question that follows:

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Which equation for the reaction at the anode is correct?

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The electrode potential of

M^{2 +} / M

3

d-series elements shows positive value for?

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An aqueous solution of nickel (II) sulphate was electrolyzed using nickel electrodes. Observe the diagram and answer the question that follows:

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Name the cation that remains as a spectator ion in the solution.

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Chemistry>Physical Chemistry>Redox Reactions>Redox Reactions and Electrode Processes

The electrode potential, $E °,$ for the reduction of ${MnO}_{4}^{-}$ to ${Mn}^{2 +}$ in acidic medium is $+ 1.51$
V. Which of the following metal(s) will be oxidised? The reduction reactions and standard electrode potentials for ${Zn}^{2 +}, {Ag}^{+}$ and ${Au}^{+}$ ${Au}^{+}$ are given as

${Zn}^{2 +} (aq) + 2 e ⟶ Zn (s), E ° = - 0.762 V$

${Ag}^{+} (aq) + e ⇌ Ag (s), E ° = + 0.80 V$

${Au}^{+} (aq) + e ⇌ Au (s), E ° + 1.69 V$

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Chemistry>Physical Chemistry>Redox Reactions>Redox Reactions and Electrode Processes

The hydrogen electrode is dipped in a solution of

pH = 3 at 25 ° C

, the potential of the cell would be (the value of

\frac{2.303 RT}{F} = 0.059 V

)

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In the following resonance structures, the curved arrow indicates that electrons are shifted from

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Chemistry>Physical Chemistry>Redox Reactions>Redox Reactions and Electrode Processes

Which of the following transformations can be carried out by using

H I

as a reducing agent, under acidic conditions?

[Given :

I_{2} (s) \to 2 I^{-} E^{o} = 0.54 V

]

(i)

C u^{+} \to C u (s) E^{o} = 0.52 V

(ii)

C r^{3 +} \to C r^{2 +} E^{o} = - 0.41 V

(iii)

F e^{3 +} \to F e^{2 +} E^{o} = 0.77 V

(iv)

F e^{2 +} \to F e (s) E^{o} = - 0.44 V

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Chemistry>Physical Chemistry>Redox Reactions>Redox Reactions and Electrode Processes

What is the standard potential of cell

Ni ∣ {Ni}^{2 +} (1 M) ‖ {Cu}^{2 +} (1 M) | Cu

{E^{o}}_{{Cu}^{+ 2} | Cu} = 0 \cdot 337 V

and

{E^{o}}_{{Ni}^{+ 2} | Ni} = - 0 \cdot 236 V

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The order of reactivity of

K, M g, A u

and

Z n

with water is

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Chemistry>Physical Chemistry>Redox Reactions>Redox Reactions and Electrode Processes

On the basis of standard electrode potential values, suggest which of the following reactions would take place?

\begin{matrix} E_{{Cu}^{2 +} | Cu}^{o} = 0.34 V, E_{{Zn}^{2 +} | Zn}^{o} = - 0.76 V, \\ E_{{Mg}^{2 +} | Mg}^{o} = - 2.37 V, E_{{Fe}^{2 +} | Fe}^{o} = - 0.74 V, \\ E_{{Br}_{2} | {Br}^{-}}^{o} = + 1.08 V, E_{{Cl}_{2} | {Cl}^{-}}^{o} = + 1.36 V \\ E_{{Cd}^{2 +} | Cd}^{o} = - 0.44 V \end{matrix}

(i)

Cu + {Zn}^{+ 2} \to {Cu}^{2 +} + Zn

(ii)

Mg + {Fe}^{2 +} \to {Mg}^{2 +} + Fe

(iii)

{Br}_{2} + 2 {Cl}^{-} \to {Cl}_{2} + 2 {Br}^{-}

(iv)

Fe + {Cd}^{2 +} \to Cd + {Fe}^{2 +}

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Chemistry>Physical Chemistry>Redox Reactions>Redox Reactions and Electrode Processes

The half-cell potentials for the metallic elements A, B, C and D are 0.8V, –0.74V, 1.1V and +0.34V respectively. Arrange these in the order of decreasing metallic character

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Chemistry>Physical Chemistry>Redox Reactions>Redox Reactions and Electrode Processes

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

\begin{matrix} E_{Cu (red)}^{\circ} = 0.34 V \\ E_{Ag (red)}^{\circ} = 0.80 V \end{matrix}

Ag⁺(aq) , Cu(s) Report the value of

E_{cell}^{o}

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Chemistry>Physical Chemistry>Redox Reactions>Redox Reactions and Electrode Processes

Using the standard electrode potentials given below, calculate the

E^{0}

cell for Fe³⁺(aq) and Cu(s)

(\begin{matrix} E_{{Fe}^{3 +} / {Fe}^{2 +}}^{\circ} = 0.77 V, & E_{{Cu}^{2 +} / Cu}^{\circ} = 0.34 V \end{matrix})

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As per study of electrochemical series, which of the following reaction is non-spontaneous?

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An aqueous solution containing one mole per litre each

Cu {({NO}_{3})}_{2} {, AgNO}_{3}, Hg {({NO}_{3})}_{2}, Mg {({NO}_{3})}_{2}

being electrolysed using inert electrode. The values of standard electrode potential in volts are:

\begin{matrix} Ag | {Ag}^{+} = + 0.80 & 2 Hg | {Hg}^{+} = + 0.79 \\ Cu | {Cu}^{+ +} = + 0.34 & Mg | {Mg}^{+ +} = - 2.37 \end{matrix}

With increasing voltage, the sequence of deposition of metal on cathode will be:

An iron wire is immersed in a solution containing ZnSO4 and NiSO4. When the concentration of each salt is 1M, predict which of the following reaction is likely to proceed. Given EoZn+2/Zn=-0.76 V EoFe+2/Fe=-0.44 V and Eo(Ni+2/Ni)=-0.25 V

Important Questions on Redox Reactions

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