For the reduction of NO 3-ion in an aqueous solution E - is -0-96 V- Values of E - for some metal ions are given below-V 2- aq -2 e - V - E 0-1-19 VF e 3- aq -3 e - Fe - E -0-04 VAu 3- aq -3 e - Au - E -1-40 VHg 2- aq -2 e - Hg - E 0-0-86 VThe pairs of metals that is-are oxidised by NO 3-in aqueous solution is areA- V and HgB- Hg and FeC- Fe and AuD- Fe and V

The correct options are A V and Hg B Hg and Fe D Fe and VMetals with E^∘ value less than 0.96 V will be able to reduce NO_3^ in aqueous solution. Therefore, me ...

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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 $E^{\circ}$ 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)

V and Hg

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Hg and Fe

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Fe and Au

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Fe and V

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Solution

The correct options are
A V and Hg
B Hg and Fe
D Fe and V
Metals with $E^{\circ}$ value less than 0.96 V will be able to reduce $N O_{3}^{-}$ in aqueous solution. Therefore, metals $V (E^{\circ} = - 1.19 V), F e (E^{\circ} = - 0.04 V), H g (E^{\circ} = 0.86 V)$ will all reduce $N O_{3}^{-}$ but $A u (E^{\circ} = 1.40 V)$ cannot reduce $N O_{3}^{-}$ in aqueous solution.

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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 $E^{0}$ 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)

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)