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Electrochemical Series

For the reduc...

Question

For the reduction of $N O_{3}^{⊖}$ ion in an aqueous solution, $E^{⊖}$ is +0.96 V, the values of $E^{⊖}$ for some metal ions are given below:
$(i) V^{2 +} (a q) + 2 e^{-} \to V; E^{⊖} = - 1.19 V$
$(i i) F e^{3 +} (a q) + 3 e^{-} \to F e; E^{⊖} = - 0.04 V$
$(i i i) A u^{3 +} (a q) + 3 e^{-} \to A u; E^{⊖} = + 1.40 V$
$(i v) H g^{2 +} (a q) + 2 e^{-} \to H g; E^{⊖} = + 0.86 V$

The pair(s) of metals that is/are oxidized by $N O_{3}^{⊖}$ in aqueous solution is/are
(IIT-JEE, 2010)

A

$F e$ and $A u$

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B

$H g$ and $F e$

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C

$V$ and $H g$

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D

$F e$ and $V$

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Solution

The correct option is D
$F e$ and $V$

The basic idea is pretty straightforward here. You need to see if a reaction is spontaneous or not. How do you do this? Calculate the overall $E^{0}$ of the reaction. If it is +ve, then the reaction would be spontanoues. Easy enough?
You just need to check with every option since this is a multiple answer correct question.

$N O_{3}^{⊖} + e^{-} \to ?; E_{r e d}^{⊖} = 0.96 V$
Compare the standard reduction potential fo the given metals with that of $N O_{3}^{⊖}$ reduction.
$E_{r e d u c t i o n}^{⊖}$ for $N O_{3}^{⊖}$ is greater than $E_{r e d u c t i o n}^{⊖}$ of (i), (ii), and (iv).
So, $N O_{3}^{⊖}$ will be able to oxidize Fe, Hg, and V.
So pairs are as in (b), (c) and (d).

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For the reduction of

N O_{3}^{-}

ion in an aqueous solution

E^{\circ}

is +0.96 V. Values of

E^{\circ}

for some metal ions are given below:

V^{2 +} (a q) + 2 e^{-} \to V; E^{0} = - 1.19 V

F e^{3 -} (a q) + 3 e^{-} \to F e; E^{\circ} = - 0.04 V

A u^{3 +} (a q) + 3 e^{-} \to A u; E^{\circ} = + 1.40 V

H g^{2 +} (a q) + 2 e^{-} \to H g; E^{0} = + 0.86 V

The pair(s) of metals that is/are oxidised by

N O_{3}^{-}

in aqueous solution is (are)

Q. For the reduction of /( NO_{3}^{\ominus } \) ion in an aqueous solution,

E^{⊖}

is +0.96 V, the values of

E^{⊖}

for some metal ions are given below:

(i) V^{2 +} (a q) + 2 e^{-} \to V; E^{⊖} = - 1.19 V

(i i) F e^{3 +} (a q) + 3 e^{-} \to F e; E^{⊖} = - 0.04 V

(i i i) A u^{3 +} (a q) + 3 e^{-} \to A u; E^{⊖} = + 1.40 V

(i v) H g^{2 +} (a q) + 2 e^{-} \to H g; E^{⊖} = + 0.86 V

The pair(s) of metals that is/are oxidized by NO_{3}^{\ominus } in aqueous solution is/are
(IIT-JEE, 2010)

Q.
For the reduction of

N O_{3}^{-}

ion in an aqueous solution

E^{\circ}

is +0.96 V. Values of

E^{\circ}

for some metal ions are given below:

V^{2 +} (a q) + 2 e^{-} \to V; E^{0} = - 1.19 V

F e^{3 -} (a q) + 3 e^{-} \to F e; E^{\circ} = - 0.04 V

A u^{3 +} (a q) + 3 e^{-} \to A u; E^{\circ} = + 1.40 V

H g^{2 +} (a q) + 2 e^{-} \to H g; E^{0} = + 0.86 V

The pair(s) of metals that is/are oxidised by

N O_{3}^{-}

in aqueous solution is (are)

Q. For the reduction of

N O_{3}^{-}

ion in an aqueous solution

E^{o}

0.96 V

E^{o}

for some metal ions are given below:

V^{2 +} (a q) + 2 e^{-} \to V; E^{o} = - 1.19 V F e^{3 +} (a q) + 3 e^{-} \to F e; E^{o} = - 0.04 V A u^{3 +} (a q) + 3 e^{-} \to A u; E^{o} = 1.40 V H g^{2 +} (a q) + 2 e^{-} \to H g; E^{o} = + 0.86 V

The pair(s) of metals that is/are oxidised by

N O_{3}^{-}

in aqueous solution is (are):

For the reduction of $N O_{3}^{-}$ ion in an aqueous solution $E^{0}$ is + 0.96 V. Values of $E^{0}$ for some metal ions are given below
$V^{2 +} (a q) + 2 e^{-} \to V; E^{0} = - 1.19 V F e^{3 +} (a q) + 3 e^{-} \to F e; E^{0} = - 0.04 V A u^{3 +} (a q) + 3 e^{-} \to A u; E^{0} = - 1.40 V H g^{2 +} (a q) + 2 e^{-} \to H g; E^{0} = - 0.86 V$
The pair (s) of metals that is/ are oxidized by $N O_{3}^{-}$ in aqueous solution is (are)

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