The more positive the value of $E^{\circ}$ , the greater is the tendency of the species to getreduced. Using the standard electrode potential of redox couples given below find outwhich of the following is the strongest oxidising agent. $E^{\circ}$ values:
$F e^{3 +} / F e^{2 +} = + 0.77; I_{2} (s) / I^{-} = + 0.54;$
$C u^{2 +} / C u = + 0.34; A g^{+} / A g = + 0.80 V$

F e^{3 +}

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I_{2} (s)

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C u^{2 +}

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A g^{+}

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Solution

The correct option is D $A g^{+}$
Given $E^{0}$ values : $F e^{3 +} / F e^{2 +} = + 0.77 V$ ; $I_{2 (s)} / I^{-} = + 0.54 V$ ; $C u^{2 +} / C u = + 0.34 V$ ; $A g^{+} / A g = + 0.80 V$
Since Strongest oxidising agent means it has greater tendency to oxidise other species and itself gets easily reduced. So higher the $E^{0}$ values, stronger is the oxidising agent it is. Thus, $A g^{+}$ having highest positive $E^{0}$ value among the given systems, is the strongest oxidising agent.

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Similar questions

Q. Using the standard electrode potential , find out the pair between which redox reaction is not feasible .

E^{0}

values :

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

= +0.77;

I_{2} / I^{-}

= + 0.54;

C u^{2 +} / C u

= +0.34;

A g^{+} / A g

= +0.80V

The more positive the value of $E^{⊖}$ , the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.

E\ominus values :

$\frac{F e^{3 +}}{F e^{2 +}} = + 0.77 \frac{I_{2} (S)}{I^{-}} = + 0.54; \frac{C u^{2 +}}{C u} = + 0.34; \frac{A g^{+}}{A g} = 0.80 V$

(a) $F e^{3 +}$
(b) $I_{2} (s)$
(c) $C u^{2 +}$
(d) $A g^{+}$

Q. On the basis of standard electrode potential of redox couples given below, find out which of the following is the strongest oxidising agent.

(E^{0} values : F e^{3 +} ∣ F e^{2 +} = + 0.77 V; I_{2} (s) ∣ I^{-} = + 0.54 V; C u^{2 +} | C u = + 0.34 V; A g^{+} ∣ A g = + 0.80 V)

E^{⊝}

values of some redox couples are given. On the basis of these values choose the correct option:

E^{⊝}

values:

B r_{2} / B r^{-} = + 1.9; A g^{+} / A g (s) = + 0.8

C u^{2 +} / C u = + 0.34; I_{2} (s) / I^{-} = 0.54

Using the standard electrode potential, find out the pair between which redox reaction is not feasible.

$E ⊖$ values :

$\frac{F e^{3 +}}{F e^{2 +}} = + 0.77 \frac{I_{2}}{I^{-}} = + 0.54; \frac{C u^{2 +}}{C u} = + 0.34 \frac{A g^{+}}{A g} = + 0.80 V$

(a) $F e^{3 +}$ and $I^{-}$
(b) $A g^{+}$ and Cu
(c) $F e^{3 +}$ and Cu
(d) Ag and $F e^{3 +}$

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