Write the reactions for the following:
$1.$ Oxidation and reduction reactions of a lead storage cell.
$2.$ Cell reaction of a $Ni-Cd$ cell.
$3.$ Anode,cathode,and overall reaction of a mercury cell.
$1.$ Oxidation and reduction reactions of a lead storage cell.
$2.$ Cell reaction of a $Ni-Cd$ cell.
$3.$ Anode,cathode,and overall reaction of a mercury cell.
$1.$ Lead storage cell:
Anode (Oxidation): $Pb(s) + SO_4^{2-}(aq) \rightarrow PbSO_4(s) + 2e^-$
Cathode (Reduction): $PbO_2(s) + SO_4^{2-}(aq) + 4H^+(aq) + 2e^- \rightarrow PbSO_4(s) + 2H_2O(l)$
$2.$ $Ni-Cd$ cell:
Cell reaction: $Cd(s) + 2Ni(OH)_3(s) \rightarrow CdO(s) + 2Ni(OH)_2(s) + H_2O(l)$
$3.$ Mercury cell:
Anode (Oxidation): $Zn(Hg) + 2OH^-(aq) \rightarrow ZnO(s) + H_2O(l) + 2e^-$
Cathode (Reduction): $HgO(s) + H_2O(l) + 2e^- \rightarrow Hg(l) + 2OH^-(aq)$
Overall reaction: $Zn(Hg) + HgO(s) \rightarrow ZnO(s) + Hg(l)$
Anode (Oxidation): $Pb(s) + SO_4^{2-}(aq) \rightarrow PbSO_4(s) + 2e^-$
Cathode (Reduction): $PbO_2(s) + SO_4^{2-}(aq) + 4H^+(aq) + 2e^- \rightarrow PbSO_4(s) + 2H_2O(l)$
$2.$ $Ni-Cd$ cell:
Cell reaction: $Cd(s) + 2Ni(OH)_3(s) \rightarrow CdO(s) + 2Ni(OH)_2(s) + H_2O(l)$
$3.$ Mercury cell:
Anode (Oxidation): $Zn(Hg) + 2OH^-(aq) \rightarrow ZnO(s) + H_2O(l) + 2e^-$
Cathode (Reduction): $HgO(s) + H_2O(l) + 2e^- \rightarrow Hg(l) + 2OH^-(aq)$
Overall reaction: $Zn(Hg) + HgO(s) \rightarrow ZnO(s) + Hg(l)$
Explore More
Similar Questions
What is the reaction occurring at the anode in a $CH_4 - O_2$ fuel cell?
Medium
View SolutionThe zinc/silver oxide cell is used in electric watches. The reaction is as follows:
$Zn(s) + Ag_2O(s) + H_2O(l) \rightarrow Zn^{2+}(aq) + 2Ag(s) + 2OH^-(aq)$
Given:
$Zn^{2+} + 2e^- \rightarrow Zn ; E^{\circ} = -0.760 \, V$
$Ag_2O + H_2O + 2e^- \rightarrow 2Ag + 2OH^- ; E^{\circ} = 0.344 \, V$
If $F = 96,500 \, C \, mol^{-1}$,the $\Delta G^{\circ}$ of the cell will be $....$ (in $kJ \, mol^{-1}$)
$Zn(s) + Ag_2O(s) + H_2O(l) \rightarrow Zn^{2+}(aq) + 2Ag(s) + 2OH^-(aq)$
Given:
$Zn^{2+} + 2e^- \rightarrow Zn ; E^{\circ} = -0.760 \, V$
$Ag_2O + H_2O + 2e^- \rightarrow 2Ag + 2OH^- ; E^{\circ} = 0.344 \, V$
If $F = 96,500 \, C \, mol^{-1}$,the $\Delta G^{\circ}$ of the cell will be $....$ (in $kJ \, mol^{-1}$)
The standard free energy change $($ in $J)$ for the reaction $3 Fe^{2+}_{(aq)} + 2 Cr_{(s)} \rightleftharpoons 2 Cr^{3+}_{(aq)} + 3 Fe_{(s)}$ given $E_{Fe^{2+}/Fe}^{\circ} = -0.44 \, V$ and $E_{Cr^{3+}/Cr}^{\circ} = -0.74 \, V$ is $(F = 96500 \, C)$.
DifficultKVPY 2014
View SolutionGive the uses of the lead storage cell.
Easy
View SolutionMark the false statement.
Easy
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo