(B) The oxidising power of a species is directly proportional to its standard reduction potential $(E^{\circ})$.Higher the value of $E^{\circ}$,greate

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$BrO_4^{-} > IO_4^{-} > ClO_4^{-}$

(B) The oxidising power of a species is directly proportional to its standard reduction potential $(E^{\circ})$.Higher the value of $E^{\circ}$,greater is the tendency to undergo reduction,and thus stronger is the oxidising power.Comparing the given values:$BrO_4^{-} (1.74 \ V) > IO_4^{-} (1.65 \ V) > ClO_4^{-} (1.19 \ V)$.Therefore,the correct order of oxidising power is $BrO_4^{-} > IO_4^{-} > ClO_4^{-}$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Difficult

Reduction potential of ions are given below:

$ClO_4^{-}$ $E^{\circ} = 1.19 \ V$

$IO_4^{-}$ $E^{\circ} = 1.65 \ V$

$BrO_4^{-}$ $E^{\circ} = 1.74 \ V$

The correct order of their oxidising power is:

JEE MAIN 2024 All JEE MAIN

A
$ClO_4^{-} > IO_4^{-} > BrO_4^{-}$
B
$BrO_4^{-} > IO_4^{-} > ClO_4^{-}$
C
$BrO_4^{-} > ClO_4^{-} > IO_4^{-}$
D
$IO_4^{-} > BrO_4^{-} > ClO_4^{-}$

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If the reduction potential is more,then

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Given standard electrode potentials:
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Hydrogen gas is not liberated when the following metal is added to dil $HCl$.

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If standard reduction potentials $(E^0)$ of $(Al^{+3}(aq)|Al(s))$, $(Fe^{+2}(aq)|Fe(s))$, $(Cu^{+2}(aq)|Cu(s))$ and $(Ag^{+1}(aq)|Ag(s))$ are $-1.66 \text{ V}$, $-0.44 \text{ V}$, $+0.34 \text{ V}$ and $+0.79 \text{ V}$ respectively, which of the following reactions is non-spontaneous?

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$ClO_4^{-}$	$E^{\circ} = 1.19 \ V$
$IO_4^{-}$	$E^{\circ} = 1.65 \ V$
$BrO_4^{-}$	$E^{\circ} = 1.74 \ V$

Reduction potential of ions are given below: $ClO_4^{-}$ $E^{\circ} = 1.19 \ V$ $IO_4^{-}$ $E^{\circ} = 1.65 \ V$ $BrO_4^{-}$ $E^{\circ} = 1.74 \ V$ The correct order of their oxidising power is:

Similar Questions

If the reduction potential is more,then

Given standard electrode potentials:$Fe^{2+} + 2e^- \to Fe; E^o = -0.440 \ V$$Fe^{3+} + 3e^- \to Fe; E^o = -0.036 \ V$The standard electrode potential $(E^o)$ for $Fe^{3+} + e^- \to Fe^{2+}$ is .............. $V$.

The standard Gibbs energy for the given cell reaction in $kJ \, mol^{-1}$ at $298 \, K$ is $Zn_{(s)} + Cu^{2+}_{(aq)} \to Zn^{2+}_{(aq)} + Cu_{(s)}$,given $E^o = 2 \, V$ at $298 \, K$ [Faraday's constant $F = 96500 \, C \, mol^{-1}$].

Hydrogen gas is not liberated when the following metal is added to dil $HCl$.

If standard reduction potentials $(E^0)$ of $(Al^{+3}(aq)|Al(s))$, $(Fe^{+2}(aq)|Fe(s))$, $(Cu^{+2}(aq)|Cu(s))$ and $(Ag^{+1}(aq)|Ag(s))$ are $-1.66 \text{ V}$, $-0.44 \text{ V}$, $+0.34 \text{ V}$ and $+0.79 \text{ V}$ respectively, which of the following reactions is non-spontaneous?

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Reduction potential of ions are given below:

$ClO_4^{-}$ $E^{\circ} = 1.19 \ V$

$IO_4^{-}$ $E^{\circ} = 1.65 \ V$

$BrO_4^{-}$ $E^{\circ} = 1.74 \ V$

The correct order of their oxidising power is:

Given standard electrode potentials:
$Fe^{2+} + 2e^- \to Fe; E^o = -0.440 \ V$
$Fe^{3+} + 3e^- \to Fe; E^o = -0.036 \ V$
The standard electrode potential $(E^o)$ for $Fe^{3+} + e^- \to Fe^{2+}$ is .............. $V$.