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Types of Redox Reactions

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:
$V^{2 +} (a q) + 2 e^{-} \to V; E^{o} = - 1.19 V F e^{3 +} (a q) + 3 e^{-} \to F e; E^{o} = - 0.04 V A u^{3 +} (a q) + 3 e^{-} \to A u; E^{o} = 1.40 V H g^{2 +} (a q) + 2 e^{-} \to H g; E^{o} = + 0.86 V$
The pair(s) of metals that is/are oxidised by $N O_{3}^{-}$ in aqueous solution is (are):

A

V and Hg

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B

Fe and Au

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C

Hg and Fe

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D

Fe and V

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Solution

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

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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)

E^{o}

for reduction of

N O_{3}^{-}

ion in aqueous solution is

+ 0.96 V

E^{o}

values for some metals are

V_{(a q)}^{2 +} + 2 e \to V E^{o} = - 0.119 V

F e_{(a q)}^{3 +} + 3 e \to F e E^{o} = - 0.40 V

A u_{(a q)}^{3 +} + 3 e \to A u E^{o} = + 1.40 V

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

Then the pairs of metals that is not oxidised by

N O_{3}^{-}

in aqueous solution is :

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)

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