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Consider figure from the above question and answer the questions (i) to (vi) given below.
Salt bridge
Salt bridge
(i) Redraw the diagram to show the direction of elctron flow.
(ii) Is silver plate the anode or cathode?
(iii) What will happen if salt bridge is removed?
(iv) When will the cell stop functioning?
(v) How will concentration of $\mathrm{Zn}^{2+}$ ions and $\mathrm{Ag}^{+}$ions be affected when the cell functions?
(vi) How will the concentration of $\mathrm{Zn}^{2+}$ ions and $\mathrm{Ag}^{+}$ ions be affected after the cell becomes 'dead'?
Salt bridge
Salt bridge
(i) Redraw the diagram to show the direction of elctron flow.
(ii) Is silver plate the anode or cathode?
(iii) What will happen if salt bridge is removed?
(iv) When will the cell stop functioning?
(v) How will concentration of $\mathrm{Zn}^{2+}$ ions and $\mathrm{Ag}^{+}$ions be affected when the cell functions?
(vi) How will the concentration of $\mathrm{Zn}^{2+}$ ions and $\mathrm{Ag}^{+}$ ions be affected after the cell becomes 'dead'?
Solution:
2529 Upvotes
Verified Answer
(i) $E^{\circ}$ is more negative for $\mathrm{Zn}$, so $\mathrm{Zn}$ undergoes oxidation and $\mathrm{Ag}^{+}$undergoes reduction. Flow of electrons is from $\mathrm{Zn}$ to $\mathrm{Ag}$
(ii) Ag is the cathode as it is the site of reduction where $\mathrm{Ag}^{+}$takes electrons from medium and deposit at cathode.
(iii) Cell potential drops to zero when salt bridge is removed and cell will stop functioning. At $E=0$ reaction reaches equilibrium.
(iv) When $E_{\text {cell }}=0$, cell stop functioning because at this condition reaction reaches to equilibrium.
(v) Concentration of $\mathrm{Zn}^{2+}$ ions will increase because $\mathrm{Zn}$ is converted into $\mathrm{Zn}^{2+}$ and concentration of $\mathrm{Ag}^{+}$ ions will decrease because $\mathrm{Ag}^{+}$is converted into $\mathrm{Ag}$.
(vi) When $E_{\text {cell }}=0$ equilibrium is reached and concentration of $\mathrm{Zn}^{2+}$ ions and $\mathrm{Ag}^{+}$will not change.
(ii) Ag is the cathode as it is the site of reduction where $\mathrm{Ag}^{+}$takes electrons from medium and deposit at cathode.
(iii) Cell potential drops to zero when salt bridge is removed and cell will stop functioning. At $E=0$ reaction reaches equilibrium.
(iv) When $E_{\text {cell }}=0$, cell stop functioning because at this condition reaction reaches to equilibrium.
(v) Concentration of $\mathrm{Zn}^{2+}$ ions will increase because $\mathrm{Zn}$ is converted into $\mathrm{Zn}^{2+}$ and concentration of $\mathrm{Ag}^{+}$ ions will decrease because $\mathrm{Ag}^{+}$is converted into $\mathrm{Ag}$.
(vi) When $E_{\text {cell }}=0$ equilibrium is reached and concentration of $\mathrm{Zn}^{2+}$ ions and $\mathrm{Ag}^{+}$will not change.
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