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Application of Electrolysis

Standard elec...

Question

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half cell reactions and their standard potentials are given below.

$M n_{4}^{-} (a q) + 8 H^{+} (a q) + 5 e^{-} \to M n^{2 +} (a q) + 4 H_{2} O (l); E^{\circ} = 1.51 V$
$C r_{2} O_{7}^{2 -} (a q) + 14 H^{+} + 6 e^{-} \to 2 C r^{3} + (a q) + 7 H_{2} O (l); E^{\circ} = 138 V$
$F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{\circ} = 0.77 V$
$C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{\circ} = 1.40 V$

Identify the incorrect statement regarding the quantitative estimation of gaseous $F e (N O_{3})_{2}$ .

A

M n O_{4}^{-}

can be used in aqueous

H C l

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B

C r_{2} O_{7}^{2 -}

can be used in aqueous

H C l

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C

M n O_{4}^{-}

can be used in aqueous

H_{2} S O_{4}

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D

C r_{2} O_{7}^{2 -}

can be used in aqueous

H_{2} S O_{4}

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Solution

The correct option is A $M n O_{4}^{-}$ can be used in aqueous $H C l$
In aqueous HCl medium,

$M n O_{4}^{-}$ can also oxidise $C l^{-}$ to $C l_{2}$

$M n O_{4}^{-} (a q) + 8 H^{+} (a q) + 5 e^{-} \to M n^{2 +} (a q) + 4 H_{2} O (l)$

$2 C l^{-} (a q) \to C l_{2} (g) + 2 e^{-}$

The standard emf of the cell made from the above two half-reactions is:

$E_{c e l l}^{0}$ $= E_{R}^{0} - E_{L}^{0}$

$= E_{M n}^{0} - E_{C l}^{0}$

$= 1.51 - 1.40$

$= 0.11 V$

Since $E_{c e l l}^{0} > 0$ , the reaction is spontaneous.

In all other cases, the redox process between the oxidising agent and medium ( $H C l$ or $H_{2} S O_{4}$ ) are non-spontaneous, would not interfere with oxidation of $F e^{2 +}$ .

Hence, option A is correct.

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Q. Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox Titration. Some half – cell reactions and their standard potential are given below:

M n O_{4}^{-} (a q) + 8 H^{+} (a q) + 5 e^{-} \to M n^{2 +} (a q) + 4 H_{2} O (I); E^{\circ} = 1.51 V

C r_{2} O_{7}^{2 -} (a q) + 14 H^{+} (a q) + 6 e^{-} \to 2 C r^{3 +} (a q) + 7 H_{2} O (I); E^{\circ} = 1.38 V

F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{\circ} = 0.77 V

C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{\circ} = 1.40 V

Identify the only incorrect statement regarding the quantitative estimation of aqueous

F e (N O_{3})_{2}

.

Q. Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox Titration. Some half – cell reactions and their standard potential are given below:

M n O_{4}^{-} (a q) + 8 H^{+} (a q) + 5 e^{-} \to M n^{2 +} (a q) + 4 H_{2} O (I); E^{\circ} = 1.51 V

C r_{2} O_{7}^{2 -} (a q) + 14 H^{+} (a q) + 6 e^{-} \to 2 C r^{3 +} (a q) + 7 H_{2} O (I); E^{\circ} = 1.38 V

F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{\circ} = 0.77 V

C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{\circ} = 1.40 V

Identify the only incorrect statement regarding the quantitative estimation of aqueous

F e (N O_{3})_{2}

.

Q. Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titrations. Some half cell reactions and their standard potentials are given below:

M n O_{4}^{-} (a q .) + 8 H^{+} (a q .) + 5 e^{-} \to M n^{2 +} (a q .) + 4 H_{2} O (l); E^{o} = 1.51 V

C r_{2} O_{7}^{2 -} (a q .) + 14 H^{+} (a q .) + 6 e^{-} \to 2 C r^{3 +} (a q .) + 7 H_{2} O (l); E^{o} = 1.38 V

F e^{3 +} (a q .) + e^{-} \to F e^{2 +} (a q .); E^{o} = 0.77 V

C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q .); E^{o} = 1.40 V

Identify the only incorrect statement regarding the quantitative estimation of aqueous

F e (N O_{3})_{2}

.

Q. Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox titration. Some half-cell reactions and their standard potentials are given below:

M n O_{4}^{-} (a q .) + 8 H^{+} (a q .) + 5 e^{-} \to M n^{2 +} (a q .) + 4 H_{2} O (l); E^{\circ} = 1.51 v o l t

C r_{2} O_{7}^{2 -} (a q .) + 14 H^{+} (a q .) + 6 e^{-} \to 2 C r^{3 +} (a q .) + 7 H_{2} O (l)^{'} E^{\circ} = 1.38 v o l t

F e^{3 +} (a q .) + e^{-} \to F e^{2 +} (a q .); E^{\circ} = 0.77 v o l t

C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q .); E^{\circ} = 1.40 v o l t

Identity the only incorrect statement regarding the quantitative estimation of aqueous

F e (N O_{3})_{2}

.

Standard electrode potential data are useful for understanding the suitability of an oxidant in a redox Titration. Some half – cell reactions and their standard potential are given below:
$M n O_{4}^{-} (a q) + 8 H^{+} (a q) + 5 e^{-} \to M n^{2 +} (a q) + 4 H_{2} O (I); E^{\circ} = 1.51 V$
$C r_{2} O_{7}^{2 -} (a q) + 14 H^{+} (a q) + 6 e^{-} \to 2 C r^{3 +} (a q) + 7 H_{2} O (I); E^{\circ} = 1.38 V$
$F e^{3 +} (a q) + e^{-} \to F e^{2 +} (a q); E^{\circ} = 0.77 V$
$C l_{2} (g) + 2 e^{-} \to 2 C l^{-} (a q); E^{\circ} = 1.40 V$

Identify the only incorrect statement regarding the quantitative estimation of aqueous $F e (N O_{3})_{2}$ .

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