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Standard XII

Chemistry

Introduction

On the basis ...

Question

On the basis of standard electrode potential of redox couples given below, find out which of the following is the strongest oxidising agent. $(E^{0} v a l u e s : F e^{3 +} | F e^{2 +} = + 0.77 V : I_{2 (s)} | I^{-} = 0.54 V; C u^{2 +} = 0.34 V; A g^{+} | A g = + 0.80 V)$

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 $A g^{+}$
Higher the reduction potential , better is the oxidising agent. Now, the reduction potential decreases in the order : $A g^{+} | A g (+ 0.80 V) > F e^{3 +} | F e^{2 +} (+ 0.77 V) > I_{2 (s)} | I^{-} (+ 0.54 V) > C u^{2 +} | C u (+ 0.34 V)$
Hence, $A g^{+}$ is the strongest oxidising agent.

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Similar questions

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)

Q. 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

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) $A g^{+}$

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

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On the basis of standard electrode potential of redox couples given below, find out which of the following is the strongest oxidising agent.(E0values:Fe3+|Fe2+=+0.77V:I2(s)|I−=0.54V;Cu2+=0.34V;Ag+|Ag=+0.80V)

The correct option is D Ag+Higher the reduction potential , better is the oxidising agent. Now, the reduction potential decreases in the order : Ag+|Ag(+0.80V)>Fe3+|Fe2+(+0.77V)>I2(s)|I−(+0.54V)>Cu2+|Cu(+0.34V)Hence, Ag+ is the strongest oxidising agent.

On the basis of standard electrode potential of redox couples given below, find out which of the following is the strongest oxidising agent. $(E^{0} v a l u e s : F e^{3 +} | F e^{2 +} = + 0.77 V : I_{2 (s)} | I^{-} = 0.54 V; C u^{2 +} = 0.34 V; A g^{+} | A g = + 0.80 V)$