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Electrochemical Series

Given Eo fo...

Question

Given $E^{o}$ for reduction of $N O_{3}^{-}$ ion in aqueous solution is $+ 0.96 V$ . If $E^{o}$ 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 :

A

V

and

H g

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B

H g

and

F e

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C

only

A u

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D

F e

and

V

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Solution

The correct option is B only $A u$
If $N O_{3}^{-}$ oxidises ant metal, then net cell emf should be positive.
As we know,
$E_{c e l l} = E_{o x i} + E_{r e d}$

So for all those cells,
$E^{o} = E_{O P_{v}}^{o} + E_{R P_{N O_{3}^{-}}}^{o} = + 1.19 + 0.96 = 2.15 V$
$E^{o} = E_{O P_{F e}}^{o} + E_{R P_{N O_{3}^{-}}}^{o} = + 0.04 + 0.96 = 1.0 V$
$E^{o} = E_{O P_{A u}}^{o} + E_{R P_{N O_{3}^{-}}}^{o} = - 1.40 + 0.96 = - 0.44 V$
$E^{o} = E_{O P_{H g}}^{o} + E_{R P_{N O_{3}^{-}}}^{o} = - 0.86 + 0.96 = + 0.10 V$

$E_{c}^{o} e l l > 0$ means reaction is spontaneous. Hence, $N O_{3}^{-}$ can't oxidise Au.

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Similar questions

Q. For the reduction of

N O_{3}^{-}

in an aqueous solution,

E^{\circ}

0.96 V

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)___________.

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 +} (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 not 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}

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)

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