Adding powdered lead and iron to a solution t | vedclass

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

Question

(B) The standard reduction potential of $Pb^{2+}|Pb$ is $E^{\circ} = -0.126 \ V$. The standard reduction potential of $Fe^{2+}|Fe$ is $E^{\circ} = -0.

Vedclass · Accepted Answer

More lead and $Fe^{2+}$ ions are formed

Vedclass · Answer

(B) The standard reduction potential of $Pb^{2+}|Pb$ is $E^{\circ} = -0.126 \ V$. The standard reduction potential of $Fe^{2+}|Fe$ is $E^{\circ} = -0.44 \ V$. Since the reduction potential of $Pb^{2+}|Pb$ is greater (less negative) than that of $Fe^{2+}|Fe$,$Pb^{2+}$ ions will be reduced to $Pb$ metal,and $Fe$ metal will be oxidized to $Fe^{2+}$ ions. The spontaneous reaction is: $Fe(s) + Pb^{2+}(aq) \rightarrow Fe^{2+}(aq) + Pb(s)$. Therefore,the addition of powdered $Pb$ and $Fe$ to the solution results in the formation of more $Pb$ and $Fe^{2+}$ ions.

Adding powdered lead and iron to a solution that is $1.0 \ M$ in both $Pb^{2+}$ and $Fe^{2+}$ ions would result in a reaction in which:

Similar Questions

In the cell represented as $Ni_{(s)}|Ni_{(1M)}^{2+}||Ag_{(1M)}^{+}|Ag_{(s)}$,the reducing agent is

The reaction at the cathode in the cells commonly used in clocks involves:

Calculate $\Delta G^{\circ}$ for the reaction $Mg_{(s)} + Sn_{(aq)}^{2+} \longrightarrow Mg_{(aq)}^{2+} + Sn_{(s)}$ if $E_{cell}^{\circ}$ is $2.23 \ V$. (in $kJ$)

On the flow of electricity,what happens to the concentration of the anode solution in a galvanic cell?

The reaction $1/2 H_{2(g)} + AgCl_{(s)} \to H^{+}_{(aq)} + Cl^{-}_{(aq)} + Ag_{(s)}$ occurs in the galvanic cell:

Vedclass Test Series

Exam Paper Generator

Online Exam Module