Which of the following reactions exhibits the | vedclass

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(C) The standard reduction potential $(E^{\circ})$ values for the given half-reactions are as follows:$1$. For $2 H_{(aq)}^{+} + 2 e^{-} \rightarrow H

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$Li_{(aq)}^{+} + e^{-} \rightarrow Li_{(s)}$

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(C) The standard reduction potential $(E^{\circ})$ values for the given half-reactions are as follows:$1$. For $2 H_{(aq)}^{+} + 2 e^{-} \rightarrow H_{2_{(g)}}$,$E^{\circ} = 0.00 \ V$.$2$. For $F_{2_{(g)}} + 2 e^{-} \rightarrow 2 F_{(aq)}^{-}$,$E^{\circ} = +2.87 \ V$.$3$. For $Li_{(aq)}^{+} + e^{-} \rightarrow Li_{(s)}$,$E^{\circ} = -3.05 \ V$.$4$. For $Cl_{2_{(g)}} + 2 e^{-} \rightarrow 2 Cl_{(aq)}^{-}$,$E^{\circ} = +1.36 \ V$.Comparing these values,the reaction involving lithium has the most negative value,which is $-3.05 \ V$. Therefore,it exhibits the minimum standard reduction potential.

Which of the following reactions exhibits the minimum standard reduction potential?

Similar Questions

If the cell potential of the cell at $298 \ K$ is $2.36 \ V$,write the cell reaction and calculate the standard electrode potential of the $Mg^{2+} \mid Mg$ half-cell.
$Mg_{(s)} \mid Mg^{2+}_{(1 \ M)} \parallel H^{+}_{(1 \ M)} \mid H_{2(g)} (1 \ bar) \mid Pt_{(s)}$

The standard oxidation potentials of zinc and silver in water at $298 \ K$ are:
$Zn_{(s)} \to Zn^{2+}_{(aq)} + 2e^- ; E^o_{ox} = 0.76 \ V$
$Ag_{(s)} \to Ag^{+}_{(aq)} + e^- ; E^o_{ox} = -0.80 \ V$
Which of the following reactions actually takes place spontaneously?

Calculate the standard potential of a cell having the following electrode reactions:
$Cd_{(aq)}^{2+} + 2e^{-} \rightarrow Cd_{(s)}$ $E^{\circ} = -0.403 \ V$
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Which method can be used to determine the strength of a reductant or oxidant in a solution? Explain with an example.

The standard electrode potential $(E^o)$ of $Cu^{2+}/Cu$ is $+0.34 \, V$,while that of $Zn^{2+}/Zn$ is $-0.76 \, V$. Explain the reason for this difference.

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