Given {E^o}_{Ag^{+}/Ag} = 0.80 V,{E^o}_{Mg^{ | vedclass

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(C) substance can be stored in a vessel if it does not react with the material of the vessel.Reaction occurs if the standard cell potential ${E^o}_{ce

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$CuCl_2$ can be stored in a silver vessel

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(C) substance can be stored in a vessel if it does not react with the material of the vessel.Reaction occurs if the standard cell potential ${E^o}_{cell} = {E^o}_{cathode} - {E^o}_{anode}$ is positive.For $AgNO_3$ in a copper vessel: $Cu + 2Ag^+ \rightarrow Cu^{2+} + 2Ag$. ${E^o}_{cell} = {E^o}_{Ag^+/Ag} - {E^o}_{Cu^{2+}/Cu} = 0.80 - 0.34 = 0.46 \ V$. Since ${E^o}_{cell} > 0$,the reaction occurs,so it cannot be stored.For $Mg(NO_3)_2$ in a copper vessel: $Cu + Mg^{2+} \rightarrow Cu^{2+} + Mg$. ${E^o}_{cell} = {E^o}_{Mg^{2+}/Mg} - {E^o}_{Cu^{2+}/Cu} = -2.37 - 0.34 = -2.71 \ V$. Since ${E^o}_{cell} For $CuCl_2$ in a silver vessel: $Ag + Cu^{2+} \rightarrow Ag^+ + Cu$. ${E^o}_{cell} = {E^o}_{Cu^{2+}/Cu} - {E^o}_{Ag^+/Ag} = 0.34 - 0.80 = -0.46 \ V$. Since ${E^o}_{cell} For $HgCl_2$ in a copper vessel: $Cu + Hg^{2+} \rightarrow Cu^{2+} + Hg$. ${E^o}_{cell} = {E^o}_{Hg^{2+}/Hg} - {E^o}_{Cu^{2+}/Cu} = 0.79 - 0.34 = 0.45 \ V$. Since ${E^o}_{cell} > 0$,the reaction occurs,so it cannot be stored.Therefore,statement $C$ is correct.

Given ${E^o}_{Ag^{+}/Ag} = 0.80 \ V$,${E^o}_{Mg^{2+}/Mg} = -2.37 \ V$,${E^o}_{Cu^{2+}/Cu} = 0.34 \ V$,${E^o}_{Hg^{2+}/Hg} = 0.79 \ V$.
Which of the following statements is correct?

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Given ${E^o}_{Ag^{+}/Ag} = 0.80 \ V$,${E^o}_{Mg^{2+}/Mg} = -2.37 \ V$,${E^o}_{Cu^{2+}/Cu} = 0.34 \ V$,${E^o}_{Hg^{2+}/Hg} = 0.79 \ V$.Which of the following statements is correct?