Which of the following metals or metal ions will be reduced by Fe- Ag-aq - e- - - Ags E- - -0-80 V Cu2- aq - 2e- - Cus E- - -0-34 V Pb2-aq - 2e- - Pbs E- - -0-13 V Fe2- aq - 2e- - Fes E- - -0-44 V Al3- aq - 3e- - Als E- - -1-66 V

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Electrochemical Series

Which of the ...

Question

Which of the following metals or metal ions will be reduced by $F e$ ?
$A g^{+} (a q) + e^{-} - > A g (s) E^{\circ} = + 0.80 V$
$C u^{2 +} (a q) + 2 e^{-} - - > C u (s) E^{\circ} = + 0.34 V$
$P b^{2 +} (a q) + 2 e^{-} - - > P b (s) E^{\circ} = - 0.13 V$
$F e^{2 +} (a q) + 2 e^{-} - - > F e (s) E^{\circ} = - 0.44 V$
$A l^{3 +} (a q) + 3 e^{-} - - > A l (s) E^{\circ} = - 1.66 V$

A g

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C u

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P b

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A l

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

E^{⊖} = - 0.44 V

A l^{3 +} + 3 e^{-} \to A l (s)

E^{⊖} = - 1.66 V

B r^{2 +} 2 e^{-} \to 2 B r^{⊖} (a q)

E^{⊖} = - 1.08 V

The oxidation and reduction half reactions of the reaction

2Al_(s) + 3Cu²⁺_(aq) → 2Al³⁺_(aq) + 3Cu_(s) are

C u

F e

E_{c e l l}^{\circ}

A l^{3 +} (a q .) + 3 e^{-} \to A l (s); E^{\circ} = - 1.66 V

C u^{2 +} (a q .) + 2 e^{-} \to C u (s); E^{\circ} = + 0.34 V

Given: $F e_{(s)} \to F e^{2 +} + 2 e^{-}; E^{o} = + 0.44 V$

$P b_{(s)} \to P b^{2 +} + 2 e^{-}; E^{o} = + 0.13 V$

$A g^{+} e^{-} \to A g; E^{o} = + 0.8 V$

$C u^{2 +} 2 e^{-} \to C u; E^{o} = + 0.34 V$

Which of the following metals will oxidise iron?

a) $A g$

b) $C u$

c) $P b$

d) None of these

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