For the reduction of ion in an aqueous solution- E - is -0-9 V value E - for some metal ions are given below-V aq -2 e - V - E -1-2 Ve aq -3-3 e - F e - E -0-05 VAu aq -3-3 e - Au - E -1-50 VHg aq -2-2 e - Hg - E -0-86 VThe metals that is are oxidised by NO 3-in aqueous solution is areA- V onlyB- V and Hg only C- V - Hg - FeD- Fe only

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Standard XII

Chemistry

Physical and Chemical Properties of Hydrogen

For the reduc...

Question

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)

V only

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V and Hg only

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V, Hg, Fe

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Fe only

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Solution

The correct option is C V, Hg, Fe
The species having more oxidation potential with respect to $N O_{3}^{-} = (E^{\circ} = - 0.96 V)$ will be oxidised by . These species are V, Fe and Hg

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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

N O_{3}^{-}

ion in an aqueous solution

E^{o}

0.96 V

. Values of

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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The correct option is C V, Hg, FeThe species having more oxidation potential with respect to NO−3=(E∘=−0.96V) will be oxidised by . These species are V, Fe and Hg

The correct option is C V, Hg, Fe
The species having more oxidation potential with respect to $N O_{3}^{-} = (E^{\circ} = - 0.96 V)$ will be oxidised by . These species are V, Fe and Hg