(D) The standard cell potential is given by the formula: ${E^0}_{cell} = {E^0}_{cathode} - {E^0}_{anode}$.Since $Cu$ has a higher reduction potential

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(D) The standard cell potential is given by the formula: ${E^0}_{cell} = {E^0}_{cathode} - {E^0}_{anode}$.Since $Cu$ has a higher reduction potential than $Mg$,$Cu$ acts as the cathode and $Mg$ acts as the anode.Thus,${E^0}_{cell} = {E^0}_{Cu^{2+}|Cu} - {E^0}_{Mg^{2+}|Mg}$.Substituting the given values: $2.7 = 0.34 - {E^0}_{Mg^{2+}|Mg}$.Rearranging the equation: ${E^0}_{Mg^{2+}|Mg} = 0.34 - 2.7$.Therefore,${E^0}_{Mg^{2+}|Mg} = -2.36 \ V$.

Class 12 Chemistry Electrochemistry Electrode potential and ECell

Medium

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?

A
$3.04$
B
$-3.04$
C
$2.36$
D
$-2.36$

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Electrode potential and ECell

What is the standard reduction potential $(E^o)$ for $Fe^{3+} \to Fe$ ? ............... $V$
Given that :
$Fe^{2+} + 2e^- \to Fe;$ $E^o_{Fe^{2+}/Fe} = -0.47 \ V$
$Fe^{3+} + e^- \to Fe^{2+};$ $E^o_{Fe^{3+}/Fe^{2+}} = +0.77 \ V$

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Electrode potential of the half cell $Hg(\ell) | Hg_2Cl_{2(s)} | Cl^-_{(aq)}$ can be increased by

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For the cell reaction,$2Ce^{4+} + Co \to 2Ce^{3+} + Co^{2+}$,$E_{cell}^o$ is $1.89 \, V$ and $E_{Co/Co^{2+}}^o = +0.28 \, V$. If $E_{Ce^{4+}/Ce^{3+}}^o = x$,then $x$ is ............. $V$.

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Which one of the following metals cannot evolve $H_2$ from acids,$H_2O$,or from its compounds?

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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.

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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?

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What is the standard reduction potential $(E^o)$ for $Fe^{3+} \to Fe$ ? ............... $V$Given that :$Fe^{2+} + 2e^- \to Fe;$ $E^o_{Fe^{2+}/Fe} = -0.47 \ V$$Fe^{3+} + e^- \to Fe^{2+};$ $E^o_{Fe^{3+}/Fe^{2+}} = +0.77 \ V$

Electrode potential of the half cell $Hg(\ell) | Hg_2Cl_{2(s)} | Cl^-_{(aq)}$ can be increased by

For the cell reaction,$2Ce^{4+} + Co \to 2Ce^{3+} + Co^{2+}$,$E_{cell}^o$ is $1.89 \, V$ and $E_{Co/Co^{2+}}^o = +0.28 \, V$. If $E_{Ce^{4+}/Ce^{3+}}^o = x$,then $x$ is ............. $V$.

Which one of the following metals cannot evolve $H_2$ from acids,$H_2O$,or from its compounds?

Which method can be used to determine the strength of a reductant or oxidant in a solution? Explain with an example.

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What is the standard reduction potential $(E^o)$ for $Fe^{3+} \to Fe$ ? ............... $V$
Given that :
$Fe^{2+} + 2e^- \to Fe;$ $E^o_{Fe^{2+}/Fe} = -0.47 \ V$
$Fe^{3+} + e^- \to Fe^{2+};$ $E^o_{Fe^{3+}/Fe^{2+}} = +0.77 \ V$