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 $F e^{2 +} (a q)$

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Solution

(i) When emf is positive, the reaction is feasible.
$E_{c e l l}^{o} = E_{F e}^{o} - E_{I_{2}}^{0} = 0.77 - 0.54 = 0.23 V$
Reaction is feasible.

(ii) $E_{c e l l}^{o} = E_{A g}^{o} - E_{C u}^{o} = 0.80 - 0.34 = 0.46 V$
Reaction is feasible.

(iii) $E_{c e l l}^{o} = E_{F e}^{o} - E_{B r_{2}}^{0} = 0.77 - 1.09 = - 0.32 V$
Reaction is not feasible.

(iv) $E_{c e l l}^{o} = E_{F e}^{o} - E_{A g}^{0} = 0.77 - 0.80 = - 0.03 V$
Reaction is not feasible.

(v) $E_{c e l l}^{o} = E_{B r_{2}}^{o} - E_{F e}^{0} = 1.09 - 0.77 = 0.32 V$
Reaction is feasible.

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Similar questions

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)

(d) Ag(s) and Fe³⁺(aq)

(e) Br₂(aq) and Fe²⁺(aq)

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

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