You visited us 2 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard X

Chemistry

Electrochemical Series

Using the sta...

Question

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

F e^{3 +} a n d I^{-}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

A g^{+} a n d C u

No worries! We‘ve got your back. Try BYJU‘S free classes today!

F e^{3 +} a n d C u

No worries! We‘ve got your back. Try BYJU‘S free classes today!

A g

and

F e^{3 +}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D $A g$ and $F e^{3 +}$
Given $E^{0}$ 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
Thus the order of getting reduced is:
$A g^{+} > F e^{3 +} > I_{2} > C u^{2 +}$
Possible reactions are:
$I_{2} + C u \to I^{-} + C u^{2 +}$ :
$F e^{3 +} + I^{-} \to F e^{2 +} + I_{2}$
$F e^{3 +} + C u \to F e^{2 +} + C u^{2 +}$
$A g^{+} + F e^{2 +} \to A g + F e^{3 +}$
$A g^{+} + I^{-} \to A g + I_{2}$
$A g^{+} + C u \to A g + C u^{2 +}$

Suggest Corrections

Similar questions

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 $F e^{3 +}$

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

Using the standard electrode potential valuesl predict if the reaction between the following is feasible :

(i) $F e^{3 +} (a q) a n d I^{-} (a q)$

(ii) $A g^{+} (a q) a n d C u (s)$

(iii) $F e^{3 +} (a q) a n d B r^{-} (a q)$

(iv) $A g (s)$ and $F e^{3 +} (a q)$

(v) $B r_{2} (a q) a n d F e^{2 +} (a q)$

Given standard electrode potentials

$E_{\frac{1}{2} \frac{t_{2}}{1^{-}}}^{\circ} = + 0.541 V E_{(\frac{C u^{2 +}}{C u})}^{\circ} = + 0.34 V E_{(\frac{1}{2} \frac{B r_{2}}{B r^{-}})}^{\circ} = + 1.09 V E_{(\frac{A g^{+}}{A g})}^{\circ} = + 0.80 V E_{(\frac{F e^{3 +}}{F e^{2 +}})}^{\circ} = + 0.77 V$

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)

and

I^{-} (a q)

(ii)

A g^{+} (a q)

and

C u (s)

(iii)

F e^{3 +} (a q)

and

B r^{-} (a q)

(iv)

A g (s)

and

F e^{3 +} (a q)

(v)

B r_{2} (a q)

and

F e^{2 +} (a q)

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) $A g^{+}$

Join BYJU'S Learning Program

Using the standard electrode potential , find out the pair between which redox reaction is not feasible .E0 values : Fe3+/Fe2+ = +0.77;I2/I− = + 0.54;Cu2+/Cu = +0.34; Ag+/Ag = +0.80V

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