For the reduction of NO3- in an aqueous solution- E- is 0-96 V- Values of E- for some metal ions are given below- Vaq2- - 2e- V E- - -1-19 V Feaq3- - 3e- Fe E- - -0-04 V Auaq3- - 3e- Au E- - -1-40 V Hgaq2- - 2e- Hg E- - - 0-86 VThe pairs of metal that is are oxidised by NO3 - in aqueous solution is are-

The correct options are A Hg and Fe C Fe and V D V and Hg E_M^n+/M^∘ for V, Fe and Hg are lower than that o ...

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Byju's Answer

Standard XII

Chemistry

Valency and Oxidation State

For the reduc...

Question

For the reduction of $N O_{3}^{-}$ in an aqueous solution, $E^{\circ}$ is $0.96 V$ . Values of $E^{\circ}$ for some metal ions are given below:
$V_{(a q)}^{2 +} + 2 e^{-} \to V E^{\circ} = - 1.19 V$
$F e_{(a q)}^{3 +} + 3 e^{-} \to F e E^{\circ} = - 0.04 V$
$A u_{(a q)}^{3 +} + 3 e^{-} \to A u E^{\circ} = + 1.40 V$
$H g_{(a q)}^{2 +} + 2 e^{-} \to H g E^{\circ} = + 0.86 V$
The pair(s) of metal that is (are) oxidised by $N O_{3}$ $^{-}$ in aqueous solution is (are)___________.

V

and

H g

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H g

and

F e

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F e

and

A u

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F e

and

V

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Solution

The correct options are
A $H g$ and $F e$
C $F e$ and $V$
D $V$ and $H g$
$E_{M^{n +} / M}^{\circ}$ for $V, F e$ and $H g$ are lower than that of $N O_{3}^{-}$ , so, $N O_{3}^{-}$ will oxidise $V, F e$ and $H g$ .

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Similar questions

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. For the reduction of ion in an aqueous solution,

E^{\circ}

is +0.9V value

E^{\circ}

for some metal ions are given below.

V_{(a q)}^{+ 2} + 2 e^{-} \to V, E^{\circ} = - 1.2 V

F e_{(a q)}^{+ 3} + 3 e^{-} \to F e, E^{\circ} = - 0.05 V

A u_{(a q)}^{+ 3} + 3 e^{-} \to A u, E^{\circ} = + 1.50 V

H g_{(a q)}^{+ 2} + 2 e^{-} \to H g, E^{\circ} = + 0.86 V

The 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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The correct options are A Hg and Fe C Fe and V D V and HgE∘Mn+/M for V,Fe and Hg are lower than that of NO−3, so, NO−3 will oxidise V,Fe and Hg.

The correct options are
A $H g$ and $F e$
C $F e$ and $V$
D $V$ and $H g$
$E_{M^{n +} / M}^{\circ}$ for $V, F e$ and $H g$ are lower than that of $N O_{3}^{-}$ , so, $N O_{3}^{-}$ will oxidise $V, F e$ and $H g$ .