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Electrochemical Series

For the reduc...

Question

For the reduction of $N O_{3}^{-}$ ion in an aqueous solution, $E^{0} i s + 0.96 V .$ 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) metals that is(are) oxidized by $N O_{3}^{-}$ in aqueous solution is(are):

A

V

and

H g

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B

H g

and

F e

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C

F e

and

A u

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D

F e

and

V

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Solution

The correct options are
A $V$ and $H g$
B $H g$ and $F e$
D $F e$ and $V$
$N O_{3}^{-}$ ion in an aqueous solution $E_{0}$ is $+ 0.96 V$ . It can oxidize only those metals that have standard reduction potentials $E^{o}$ less than $N O_{3}^{-}$ .

Thus, the metal $V, F e$ and $H g$ can be oxidized by $N O_{3}^{-}$ but not $A u$ .

Options A, B, and D are correct.

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Similar questions

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

F e^{3 +} (aq) + 3 e^{-} \to F e E^{0} = - 0.04 V

A u^{3 +} (aq) + 3 e^{-} \to A u E^{0} = + 1.40 V

H g^{2 +} (aq) + 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^{\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^{\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)

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)

Q. Which of the following pair of metals that is/are oxidized by

N O_{3}^{-}

in aqueous solution?

For the reduction of

N O_{3}^{-}

ion in an aqueous solution,

E^{0}

+ 0.96 V

E^{0}

for metal ions are given below.

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

F e^{3 +} (a q) + 3 e^{-} \to F e (s); E^{0} = - 0.04 V

A u^{3 +} (a q) + 3 e^{-} \to A u (s); E^{0} = + 1.40 V

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

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