Using the standard reduction potentials of th | vedclass

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Question

(A) The standard reduction potentials are: $E^{\circ}_{Li^+/Li} = -3.05 \ V$,$E^{\circ}_{Mg^{2+}/Mg} = -2.36 \ V$,$E^{\circ}_{Zn^{2+}/Zn} = -0.76 \ V$

Vedclass · Accepted Answer

$Mg$ displaces $Zn$ from its solution.

Vedclass · Answer

(A) The standard reduction potentials are: $E^{\circ}_{Li^+/Li} = -3.05 \ V$,$E^{\circ}_{Mg^{2+}/Mg} = -2.36 \ V$,$E^{\circ}_{Zn^{2+}/Zn} = -0.76 \ V$,and $E^{\circ}_{Ni^{2+}/Ni} = -0.25 \ V$. $A$ metal with a more negative reduction potential acts as a stronger reducing agent and can displace a metal with a less negative (or more positive) reduction potential from its salt solution. Comparing the values: $E^{\circ}_{Mg^{2+}/Mg} (-2.36 \ V) Since $Mg$ has a lower reduction potential than $Zn$,$Mg$ can displace $Zn$ from its solution. Therefore,the statement '$Mg$ displaces $Zn$ from its solution' is correct.

Using the standard reduction potentials of the electrodes $Li$,$Zn$,$Mg$,and $Ni$ as $-3.05 \ V$,$-0.76 \ V$,$-2.36 \ V$,and $-0.25 \ V$ respectively,identify the correct statement.

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