(A) An electrochemical cell functions as a galvanic cell when the external potential is less than $E_{\text{cell}}^0$. When an external potential grea

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Applying an external opposite potential greater than $E_{\text{cell}}^0$

(A) An electrochemical cell functions as a galvanic cell when the external potential is less than $E_{\text{cell}}^0$. When an external potential greater than $E_{\text{cell}}^0$ is applied in the opposite direction,the flow of electrons is reversed,and the cell acts as an electrolytic cell.

Class 12 Chemistry Electrochemistry Electrochemical cells

Medium

How can an electrochemical cell be converted into an electrolytic cell?

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A
Applying an external opposite potential greater than $E_{\text{cell}}^0$
B
Reversing the flow of ions in salt bridge.
C
Applying an external opposite potential lower than $E_{\text{cell}}^0$.
D
Exchanging the electrodes at anode and cathode.

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Why is an external $emf$ of more than $2.2 \ V$ required for the extraction of $Cl_2$ from brine?

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For the cell $Cu_{(s)} | Cu^{2+}_{(aq)} (1 \ M) || Zn^{2+}_{(aq)} (1 \ M) | Zn_{(s)}$,given $E^{\circ}_{Zn^{2+}/Zn} = -0.76 \ V$ and $E^{\circ}_{Cu^{2+}/Cu} = 0.34 \ V$,the cell reaction is:

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Depict the galvanic cell in which the reaction $Zn_{(s)} + 2Ag^{+}_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2Ag_{(s)}$ takes place. Further show:
$(i)$ Which of the electrode is negatively charged?
$(ii)$ The carriers of the current in the cell.
$(iii)$ Individual reaction at each electrode.

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Which substance is used as cathode in a mercury cell?

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What is a galvanic cell? Give the half-cell reactions of a Daniell cell and explain a redox couple.

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How can an electrochemical cell be converted into an electrolytic cell?

Similar Questions

Why is an external $emf$ of more than $2.2 \ V$ required for the extraction of $Cl_2$ from brine?

For the cell $Cu_{(s)} | Cu^{2+}_{(aq)} (1 \ M) || Zn^{2+}_{(aq)} (1 \ M) | Zn_{(s)}$,given $E^{\circ}_{Zn^{2+}/Zn} = -0.76 \ V$ and $E^{\circ}_{Cu^{2+}/Cu} = 0.34 \ V$,the cell reaction is:

Depict the galvanic cell in which the reaction $Zn_{(s)} + 2Ag^{+}_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2Ag_{(s)}$ takes place. Further show:$(i)$ Which of the electrode is negatively charged?$(ii)$ The carriers of the current in the cell.$(iii)$ Individual reaction at each electrode.

Which substance is used as cathode in a mercury cell?

What is a galvanic cell? Give the half-cell reactions of a Daniell cell and explain a redox couple.

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Depict the galvanic cell in which the reaction $Zn_{(s)} + 2Ag^{+}_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2Ag_{(s)}$ takes place. Further show:
$(i)$ Which of the electrode is negatively charged?
$(ii)$ The carriers of the current in the cell.
$(iii)$ Individual reaction at each electrode.