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Application of Electrolysis

Which of the ...

Question

Which of the following metal cannot be oxidized by $N O_{3}^{-}$ in aqueous solution?

For the reduction of $N O_{3}^{-}$ ion in an aqueous solution, $E^{0}$ is $+ 0.96 V$ .

$E^{0}$ for metal ions are given below.
$V^{2 +} (a q) + 2 e^{-} \to V (s); E^{0} = - 1.19 V$
$F e^{3 +} (a q) + 3 e^{-} \to F e (s); E^{0} = - 0.04 V$
$A u^{3 +} (a q) + 3 e^{-} \to A u (s); E^{0} = + 1.40 V$
$H g^{2 +} (a q) + 2 e^{-} \to H g (s); E^{0} = + 0.86 V$

A

V

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B

H g

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C

F e

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D

A u

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Solution

The correct option is D $A u$
$E^{0}$ value for the reduction of $N O_{3}^{-}$ is $0.96 V$
For a metal to get oxidised by $N O_{3}^{-}$ , the standard reduction potential of the metal should be lower than the reduction potential of $N O_{3}^{-}$ .

From the given standard reduction potentials, all the metals have lower reduction potential than $N O_{3}^{-}$ except $A u$

Hence, $A u^{3 +}$ cannot be oxidised by $N O_{3}^{-}$

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Similar questions

Q. For the reduction of

N O_{3}^{-}

ion in an aqueous solution,

E^{o}

+ 0.96 V

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)

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 $E^{0}$ 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)

Q. For the reduction of

N O_{3}^{-}

ion in an aqueous solution,

E^{0} i s + 0.96 V .

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):

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