The reducing ability of the metals K,Au,Zn an | vedclass

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(D) The reducing ability of metals is determined by their standard reduction potentials $(E^{\circ})$. $A$ metal with a more negative standard reducti

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$K > Zn > Pb > Au$

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(D) The reducing ability of metals is determined by their standard reduction potentials $(E^{\circ})$. $A$ metal with a more negative standard reduction potential is a stronger reducing agent.The standard reduction potentials $(E^{\circ})$ for the given metals are:$K^+ + e^- \rightarrow K$ $(E^{\circ} = -2.93 \ V)$$Zn^{2+} + 2e^- \rightarrow Zn$ $(E^{\circ} = -0.76 \ V)$$Pb^{2+} + 2e^- \rightarrow Pb$ $(E^{\circ} = -0.13 \ V)$$Au^{3+} + 3e^- \rightarrow Au$ $(E^{\circ} = +1.50 \ V)$Since the reducing ability increases as the standard reduction potential becomes more negative,the order of reducing ability is $K > Zn > Pb > Au$.

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

The reducing ability of the metals $K$,$Au$,$Zn$ and $Pb$ follows the order

Similar Questions

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:

From the given values,which one is a strong oxidizing agent?
$[Fe(CN)_6]^{4-} \to [Fe(CN)_6]^{3-} + e^-, E^o = -0.35 \ V$
$Fe^{2+} \to Fe^{3+} + e^-, E^o = -0.77 \ V$

The standard cell potential of a cell consisting of copper and $Mg$ standard half-cells is $2.7 \ V$. If the standard reduction potential of the copper electrode is $+0.34 \ V$,what is the standard reduction potential of the magnesium electrode in volts?

For a closed circuit Daniell cell,which of the following plots is the accurate one at a given temperature?

The cell potential of the given cell is $0.34 \, V$. Write the cell reaction and calculate $E^o_{Cu^{2+}|Cu}$.
$Pt_{(s)} \mid H_{2(g)} (1 \, bar) \mid H^+_{(1 \, M)} \parallel Cu^{2+}_{(1 \, M)} \mid Cu_{(s)}$

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