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EMF

For the cell ...

Question

For the cell $Z n (s) | Z n^{2 +} (a q) | | M^{x +} (a q) | M (s)$ , different half cells and their standard electrode potentials are given below:

$M^{x +} (a q / M (s))$ $A u^{3 +} (a q) / A u (s)$ $A g^{+} / A g (s)$ $F e^{3 +} (a q) / F e^{2 +} (a q)$ $F e^{2 +} (a q) / F e (s)$
$E_{M^{x +} / M^{/ (V)}}^{o}$
$1.40$ $0.80$ $0.77$ $- 0.44$

If $E_{Z n^{2 +} / Z n}^{o} = - 0.76 V$ , which cathode will give a maximum value of $E_{c e l l}^{o}$ per electron transferred ?

A

F e^{3 +} / F e^{2 +}

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B

A g^{+} / A g

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C

A u^{3 +} / A u

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D

F e^{2 +} / F e

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Solution

The correct option is A $A u^{3 +} / A u$
We have,

$E_{c e l l}^{0} = E_{c a t h o d e}^{0} - E_{a n o d e}^{0}$

For a high value of $E_{c e l l}^{0}$ the value of SRP of cathode should be high.

Here the highest value is for $A u^{3 +} / A u$
$E_{c e l l}^{0} = 1.4 - (- 0.76) = 2.16 V$
Note: Here the transfer of electron in the cell won't affect the $E_{c e l l}^{o}$ value.

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Similar questions

Q. What will be the

E^{0}

value for the given half cell reaction?

F e^{3 +} (a q) + 3 e^{-} \to F e (s)

E^{0}

value for the half cell reaction,

F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{0} = 0.77 V

F e^{2 +} (a q) + 2 e^{-} \to F e (s); E^{0} = - 0.44 V

Q. Using the standard electrode potentials given in Table

3.1

, predict if the reaction between the following is feasible:
(i)

F e^{3 +} (a q)

I^{-} (a q)

A g^{+} (a q)

C u (s)

F e^{3 +} (a q)

B r^{-} (a q)

A g (s)

F e^{3 +} (a q)

B r_{2} (a q)

F e^{2 +} (a q)

Using the standard electrode potentials given in the Table 8.1, predict if the reaction between the following is feasible:

(a) Fe³⁺(aq) and I^–(aq)

(b) Ag⁺(aq) and Cu(s)

(c) Fe³⁺ (aq) and Cu(s)

(d) Ag(s) and Fe³⁺(aq)

(e) Br₂(aq) and Fe²⁺(aq)

Q. Given the standard oxidation potentials:

E_{F e (s) / F e^{2 +} (a q)}^{0} = 0.44 V

E_{F e^{2 +} (a q) / F e^{3 +} (a q)}^{0} = - 0.77 V

The standard EMF of the given reaction will be:

F e (s) + 2 F e^{3 +} (a q) \to 3 F e^{2 +} (a q)

E_{F e^{3 +} / F e}^{0} = 0.036 V, E_{F e^{2 +} / F e}^{0} = - 0.439 V

. The value of standard electrode potential for the change,

F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q)

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