(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:

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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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Electrode potential and ECell

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Aluminium displaces hydrogen from acids but copper does not. $A$ galvanic cell prepared by combining $Cu/Cu^{2+}$ and $Al/Al^{3+}$ has an e.m.f. of $2.0 \ V$ at $298 \ K$. If the potential of copper electrode is $+0.34 \ V$,that of aluminium is .......... $V$

Medium

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Electrode potentials $(E^o)$ are given below:
$Cu^{+}/Cu = +0.52 \ V$
$Fe^{3+}/Fe^{2+} = +0.77 \ V$
$\frac{1}{2} I_{2(s)}/I^{-} = +0.54 \ V$
$Ag^{+}/Ag = +0.88 \ V$
Based on the above potentials,the strongest oxidizing agent will be:

DifficultJEE MAIN 2013

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The relation between $\Delta G$ and $E$ for a cell is $\Delta G = -nFE$. The cell reaction will be spontaneous if:

Easy

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At ${25 \, ^\circ C}$,the standard reduction potentials for $Li^+/Li$,$Ba^{2+}/Ba$,$Na^+/Na$,and $Mg^{2+}/Mg$ are $-3.05 \, V$,$-2.73 \, V$,$-2.71 \, V$,and $-2.36 \, V$ respectively. Which of the following is the strongest oxidizing agent?

Medium

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For the feasibility of a redox reaction in a cell,the e.m.f. should be

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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

Aluminium displaces hydrogen from acids but copper does not. $A$ galvanic cell prepared by combining $Cu/Cu^{2+}$ and $Al/Al^{3+}$ has an e.m.f. of $2.0 \ V$ at $298 \ K$. If the potential of copper electrode is $+0.34 \ V$,that of aluminium is .......... $V$

Electrode potentials $(E^o)$ are given below:$Cu^{+}/Cu = +0.52 \ V$$Fe^{3+}/Fe^{2+} = +0.77 \ V$$\frac{1}{2} I_{2(s)}/I^{-} = +0.54 \ V$$Ag^{+}/Ag = +0.88 \ V$Based on the above potentials,the strongest oxidizing agent will be:

The relation between $\Delta G$ and $E$ for a cell is $\Delta G = -nFE$. The cell reaction will be spontaneous if:

At ${25 \, ^\circ C}$,the standard reduction potentials for $Li^+/Li$,$Ba^{2+}/Ba$,$Na^+/Na$,and $Mg^{2+}/Mg$ are $-3.05 \, V$,$-2.73 \, V$,$-2.71 \, V$,and $-2.36 \, V$ respectively. Which of the following is the strongest oxidizing agent?

For the feasibility of a redox reaction in a cell,the e.m.f. should be

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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:

Electrode potentials $(E^o)$ are given below:
$Cu^{+}/Cu = +0.52 \ V$
$Fe^{3+}/Fe^{2+} = +0.77 \ V$
$\frac{1}{2} I_{2(s)}/I^{-} = +0.54 \ V$
$Ag^{+}/Ag = +0.88 \ V$
Based on the above potentials,the strongest oxidizing agent will be: