For the reduction of NO3- ion in an aqueous solution- Eo is -0-96 V- Values of Eo for some metal ions are given below-V2- aq-2e- V E0 - -1-19 VFe3- aq-3e- Fe E0 - -0-04 V-Au3- aq-3e- Au E0 - -1-40 V-Hg2- aq-2e- Hg E0 - -0-86 VThe pairs of metals that is are oxidised by NO3- in aqueous solution is are

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Standard IX

Chemistry

Electrochemical Series

For the reduc...

Question

For the reduction of $N O_{3}^{-}$ ion in an aqueous solution, $E^{o}$ is $+ 0.96 V$ . Values of $E^{o}$ 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)

V and H g

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F e and H g

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F e and A u

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F e and V

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Solution

The correct option is D $F e and V$
The species having less reduction potential with respect to $N O_{3}^{-}$ $(E^{o} = + 0.96 V)$ will be oxidised by $N O_{3}^{-}$ . Here $V, F e, and H g$ has less reduction potential value compared to $N O_{3}^{-}$ . Thus $V, F e, and H g$ will get oxidised by $N O_{3}^{-}$

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Similar questions

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

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)

Q. 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):

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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The correct option is D Fe and VThe species having less reduction potential with respect to NO−3 (Eo=+0.96 V) will be oxidised by NO−3. Here V, Fe, and Hg has less reduction potential value compared to NO−3. Thus V, Fe, and Hg will get oxidised by NO−3