In which metal container can an aqueous solut | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(C) To store an aqueous solution of $CuSO_4$,the metal of the container must not react with $Cu^{2+}$ ions. $A$ reaction will occur if the reduction p

Vedclass · Accepted Answer

$Ag$

Vedclass · Answer

(C) To store an aqueous solution of $CuSO_4$,the metal of the container must not react with $Cu^{2+}$ ions. $A$ reaction will occur if the reduction potential of the container metal is lower than that of $Cu^{2+}/Cu$ $(0.34 \ V)$. The reduction potentials $(E^0_{M^{n+}/M})$ are: $E^0_{Fe^{2+}/Fe} = -0.44 \ V$ $E^0_{Ni^{2+}/Ni} = -0.25 \ V$ $E^0_{Al^{3+}/Al} = -1.66 \ V$ $E^0_{Ag^{+}/Ag} = 0.80 \ V$ For the reaction $M + Cu^{2+} \rightarrow M^{n+} + Cu$ to be non-spontaneous,the $E^0_{cell}$ must be negative. $E^0_{cell} = E^0_{cathode} - E^0_{anode} = E^0_{Cu^{2+}/Cu} - E^0_{M^{n+}/M}$. For $E^0_{cell}  E^0_{Cu^{2+}/Cu}$. Comparing values,only $Ag$ has a reduction potential $(0.80 \ V)$ greater than $Cu$ $(0.34 \ V)$. Therefore,$CuSO_4$ can be stored in an $Ag$ container.

In which metal container can an aqueous solution of $CuSO_4$ be stored?
$E^0_{Cu^{2+}/Cu} = 0.34 \ V$,$E^0_{Fe/Fe^{2+}} = 0.44 \ V$,$E^0_{Al/Al^{3+}} = 1.66 \ V$,$E^0_{Ni/Ni^{2+}} = 0.25 \ V$,$E^0_{Ag^{+}/Ag} = 0.80 \ V$

Similar Questions

The $E^0_{cell}$ of the cell $Al(s)|Al^{3+}(1M)||Pb^{2+}(1M)|Pb(s)$ is $1.5 \text{ V}$. If $E^0_{Pb^{2+}/Pb}$ is $-0.14 \text{ V}$, then the standard electrode potential $E^0_{Al^{3+}/Al}$ will be: (in $\text{ V}$)

Two half-cell reactions are given below:
$Co^{3+} + e^- \rightarrow Co^{2+}, E^{\circ}_{Co^{3+}/Co^{2+}} = 1.81 \, V$
$Al^{3+} + 3e^- \rightarrow Al(s), E^{\circ}_{Al^{3+}/Al} = -1.66 \, V$
The standard $EMF$ of a cell with a feasible redox reaction will be:

The standard electrode potential of $M^{+} / M$ in aqueous solution does not depend on

Calculate the $emf$ of the cell $Cu_{(s)} | Cu^{2+}_{(aq)} || Ag^+_{(aq)} | Ag_{(s)}$. Given: $E^0_{Cu^{2+}/Cu} = +0.34 \ V$,$E^0_{Ag^+/Ag} = +0.80 \ V$.

What happens to the Gibbs free energy in a spontaneous electrochemical process?

Vedclass Test Series

Exam Paper Generator

Online Exam Module

In which metal container can an aqueous solution of $CuSO_4$ be stored? $E^0_{Cu^{2+}/Cu} = 0.34 \ V$,$E^0_{Fe/Fe^{2+}} = 0.44 \ V$,$E^0_{Al/Al^{3+}} = 1.66 \ V$,$E^0_{Ni/Ni^{2+}} = 0.25 \ V$,$E^0_{Ag^{+}/Ag} = 0.80 \ V$