The standard reduction potentials $E^{0}$ of the following systems are

System $E^{0}$ volts

(i) $M n O_{4}^{-} + 8 H^{+} + 5 e^{-} ⟶ M n^{2 +} + 4 H_{2} 0$ 1.51

(ii) $S n^{4 +} + 2 e^{-} ⟶ S n^{2 +}$ 0.15

(iii) $C r_{2} O_{7}^{2 -} + 14 H^{+} + 6 e^{-} ⟶ 2 C r^{3 +} + 7 H_{2} O$ 1.33

(iv) $C e^{4 +} + e^{-} ⟶ C e^{3 +}$ 1.61

The oxidising power of the various species decreases in the order

C e^{4 +} > C r_{2} O_{7}^{2 -} > S n^{4 +} > M n O_{4}^{-}

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C e^{4 +} > M n O_{4}^{-} > C r_{2} O_{7}^{2 -} > S n^{4 +}

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C r_{2} O_{7}^{2 -} > S n^{4 +} > C e^{4 +} > M n O_{4}^{-}

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M n O_{4}^{-} > C e^{4 +} > S n^{4 +} > C r_{2} O_{7}^{2 -}

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Solution

The correct option is B $C e^{4 +} > M n O_{4}^{-} > C r_{2} O_{7}^{2 -} > S n^{4 +}$
The higher the standard reduction potential, the higher is the oxidising power.
$Reduction Potential \propto Oxidising Power$
The standard reduction potential order is $C e^{4 +} > M n O_{4}^{-} > C r_{2} O_{7}^{2 -} > S n^{4 +}$ . thus same will be order of oxidising power. Hence option (b) is correct.

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Similar questions

Q. The standard redox potentials E

^{o}

of the following systems are:

	System	E $^{o}$ (volts)
(i)	$M n O_{4}^{-} + 8 H^{+} + 5 e^{-} \to M n^{2 +} + 4 H_{2} O$	1.51
(ii)	$S n^{2 +} \to S n^{4 +} + 2 e^{-}$	0.15
(iii)	$C r_{2} O_{7}^{2 -} + 14 H^{+} + 6 e^{-} \to 2 C r^{3 +} + 7 H_{2} O$	1.33
(iv)	$C e^{3 +} \to C e^{4 +} + e^{-}$	1.61

The oxidising power of the various species are related as:

Q. The standard redox potentials

E^{0}

of the following system are

I . M n O_{4}^{-} + 8 H^{+} + 5 e^{-} \to M n^{2 +} + 4 H_{2} O E^{0} = 1.5 V

I I . S n^{2 +} \to S n^{4 +} + 2 e^{-} E^{0} = - 0.15 V

I I I . C r_{2} O_{7}^{2 -} + 14 H^{+} + 6 e^{-} \to 2 C r^{2 +} + 7 H_{2} O E^{0} = 1.33 V

I V . C e^{3 +} \to C e^{4 +} + e^{-} E^{0} = - 1.61 V

The oxidizing power of the various species are related as

Q. The standard redox potentials

E^{0}

of the following system are

I . M n O_{4}^{-} + 8 H^{+} + 5 e^{-} \to M n^{2 +} + 4 H_{2} O E^{0} = 1.5 V

I I . S n^{2 +} \to S n^{4 +} + 2 e^{-} E^{0} = - 0.15 V

I I I . C r_{2} O_{7}^{2 -} + 14 H^{+} + 6 e^{-} \to 2 C r^{2 +} + 7 H_{2} O E^{0} = 1.33 V

I V . C e^{3 +} \to C e^{4 +} + e^{-} E^{0} = - 1.61 V

The oxidizing power of the various species are related as

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_{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}

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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	System	$E^{0}$ volts
(i)	$M n O_{4}^{-} + 8 H^{+} + 5 e^{-} ⟶ M n^{2 +} + 4 H_{2} 0$	1.51
(ii)	$S n^{4 +} + 2 e^{-} ⟶ S n^{2 +}$	0.15
(iii)	$C r_{2} O_{7}^{2 -} + 14 H^{+} + 6 e^{-} ⟶ 2 C r^{3 +} + 7 H_{2} O$	1.33
(iv)	$C e^{4 +} + e^{-} ⟶ C e^{3 +}$	1.61

The standard reduction potentials E0 of the following systems are System E0volts (i) MnO−4+8H++5e−⟶Mn2++4H20 1.51 (ii) Sn4++2e−⟶Sn2+ 0.15 (iii) Cr2O2−7+14H++6e−⟶2Cr3++7H2O 1.33 (iv) Ce4++e−⟶Ce3+ 1.61 The oxidising power of the various species decreases in the order