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Electrochemical Series

The standard ...

Question

The standard electrode potentials of the electrodes are given below. Arrange them in decreasing order of ease of oxidation:
$(a) E l e c t r o d e - I, E^{o} = - 2.89 V$
$(b) E l e c t r o d e - I I, E^{o} = - 0.16 V$
$(c) E l e c t r o d e - I I I, E^{o} = 0.77 V$
$(d) E l e c t r o d e - I V, E^{o} = - 2.93 V$
$(e) E l e c t r o d e - V, E^{o} = - 1.67 V$

A

c b e a d

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B

d a e b c

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C

c e a d b

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D

c b a d e

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Solution

The correct option is B $d a e b c$
The standard electrode potential is the tendency for a chemical species to be reduced, and is measured in volts at standard conditions. The more positive the potential is the more likely it will be reduced and more negative the potential is the more likely it will be oxidized. As $(d) E l e c t r o d e - I V, E^{o} = - 2.93 V$ has highest negative value thus will be first oxidized and $(c) E l e c t r o d e - I I I, E^{o} = 0.77 V$ will be oxidized last.

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Q. Pairs of electrodes and their corresponding standard electrode potentials are given. Arrange the cells constructed by these electrodes in increasing order of emf values.

(a) E l e c t r o d e \to A, E^{o} = - 2.92 V

E l e c t r o d e \to B, E^{o} = - 2.71 V

(b) E l e c t r o d e \to C, E^{o} = - 0.760 V

E l e c t r o d e \to D, E^{o} = - 0.44 V

(c) E l e c t r o d e \to B, E^{o} = - 2.71 V

E l e c t r o d e \to D, E^{o} = - 0.44 V

(d) E l e c t r o d e \to A, E^{o} = - 2.92 V

E l e c t r o d e \to C, E^{o} = - 0.76 V

Q. The standard electrode potentials of the electrodes are given below. Arrange them in decreasing order of ease of oxidation.
(a) Electrode - I,

E^{\circ} = - 2.89 V

(b) Electrode - II,

E^{\circ} = - 0.93 V

(c) Electrode - III,

E^{\circ} = 0.77 V

(d) Electrode - IV,

E^{\circ} = - 2.93 V

(e) Electrode - V,

E^{\circ} = - 1.67 V

Q. From the standard electrode potential values of the electrodes given select an option representing their decreasing order discharge potential:

(a) A, E^{o} = 2.32 V

(b) B, E^{o} = 1.36 V

(c) C, E^{o} = 1.07 V

(c) D, E^{o} = 0.43 V

Q. Given, standard electrode potentials,

F e^{2 +} + 2 e^{-} \to F e, E^{o} = - 0.440

F e^{3 +} + 3 e^{-} \to F e, E^{o} = - 0.036

The standard electrode potential

(E^{o})

F e^{3 +} + e^{-} \to F e^{2 +}

Q. Given standard electrode potentials :

{F e}^{3 +} + {3 e}^{-} ⟶ F e; E^{o} = - 0.036 v o l t

{F e}^{2 +} + {2 e}^{-} ⟶ F e; E^{o} = - 0.440 v o l t

The standard electrode potential

E^{o}

{F e}^{3 +} + e^{-} ⟶ {F e}^{2 +}

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