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

EASY

Earn 100

How many of the following will have negative standard reduction potentials?

$K, Na, Ag, Zn, Li, Cu, Hg$

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Important Questions on Redox Reactions

MEDIUM

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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

HARD

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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

Question Image

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

HARD

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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

Question Image

What do you observe at the cathode and anode respectively?

MEDIUM

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

Among the following, which is the strongest oxidizing agent?

EASY

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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

MEDIUM

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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

)

HARD

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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

Question Image

Which equation for the reaction at the anode is correct?

EASY

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

Hypophosphorus acid is a good reducing agent because

MEDIUM

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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

EASY

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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

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

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

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

EASY

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

The electrode potential of

M^{2 +} / M

3

d-series elements shows positive value for?

EASY

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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

EASY

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

The order of reactivity of

K, M g, A u

and

Z n

with water is

MEDIUM

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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

MEDIUM

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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 +}

EASY

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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

MEDIUM

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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}

EASY

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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})

EASY

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

When an iron object is plated with tin, tin does not act as sacrificial anode in protecting against corrosion, because

EASY

Chemistry>Physical Chemistry>Redox Reactions>Redox Reaction and Electrode Potential

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

How many of the following will have negative standard reduction potentials? K, Na, Ag, Zn, Li, Cu, Hg

Important Questions on Redox Reactions

Learn and Prepare for any exam you want !

How many of the following will have negative standard reduction potentials?

$K, Na, Ag, Zn, Li, Cu, Hg$