How can an electrochemical cell be converted into an electrolytic cell?
- AApplying an external opposite potential greater than $E_{\text{cell}}^0$
- BReversing the flow of ions in salt bridge.
- CApplying an external opposite potential lower than $E_{\text{cell}}^0$.
- DExchanging the electrodes at anode and cathode.
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Which of the following reactions is correct for a given electrochemical cell at $25^{\circ} C$ ?
$Pt | Br_{2(g)} | Br_{(aq)}^{-} || Cl_{(aq)}^{-} | Cl_{2(g)} | Pt$
$Pt | Br_{2(g)} | Br_{(aq)}^{-} || Cl_{(aq)}^{-} | Cl_{2(g)} | Pt$
$A$ galvanic cell has an electrical potential of $1.1 \ V$. If an opposing potential of $1.1 \ V$ is applied to this cell,what will happen to the cell reaction and the current flowing through the cell?
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View SolutionWrite the cell reaction of a lead storage battery when it is discharged. How does the density of the electrolyte change when the battery is discharged?
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View Solution$A$ hypothetical galvanic cell is $A_{(s)} | A^{+}_{(1 \ M)} || B^{+2}_{(1 \ M)} | B_{(s)}$ and the $EMF$ of the cell is positive. What is the possible cell reaction?
Which of the following is $NOT$ an example of a secondary voltaic cell?
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