Question

Given: $E_{A{g}^{+}/Ag}^o=0.80V,E_{M{g}^{2+}/Mg}^o=-2.37V,E_{C{u}^{2+}/Cu}^o=0.34V,E_{H{g}^{2+}/Hg}^o=0.79V$.
Which of the following statement is correct?

• A. $AgN{O}_3$ can be stored in copper vessel
• B. $Mg(N{O}_3{)}_2$ can not be stored in copper vessel
• C. $CuC{l}_2$ can be stored in silver vessel
• D. $HgC{l}_2$ can be stored in copper vessel

Answer 1

The correct option is A $AgN{O}_3$ can be stored in copper vessel

${E^0}_{{Ag}^{+}/Ag}=0.80V,{E^0}_{{Mg}^{2+}/mg}=-2.37V$

${E^0}_{{Cu}^{2+}/Cu}=0.34V,{E^0}_{{Hg}^{2+}/Hg}=0.79V$

The order of molecule to stay in its oxidised form is (less the potential, more tendency to stay M oxidised form)

i.e. ${Mg}^{2+}>{Cu}^{2+}>{Hg}^{2+}>{Ag}^{+}$

(most oxidised form) (most reduced form)

$\therefore Ag{NO}_3$

can't be stored $M$ Cu$vesselas$Ag$ will get reduced.

$Mg{\left({NO}_3\right)}_2$ can be stored $M$ $Cu$ vessel

The ans is :- ${CuCl}_2$ can be stored $M$ silver metal.

as ${E^0}_{cell}=-ve$

for this reaction.