Electrochemical Cells or Galvanic Cells
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CHXII03:ELECTROCHEMISTRY

330044 The electro-chemical cell stops working after some time because

1 Electrode potentials of both electrodes become zero
2 Electrode potentials of both electrodes become equal
3 Temperature of the cell increases
4 The reaction starts proceeding in opposite direction
CHXII03:ELECTROCHEMISTRY

330045 How can an electrochemical cell be converted into an electrolytic cell?

1 Exchanging the electrodes at anode and cathode.
2 Applying an external opposite potential greater than \({\mathrm{\mathrm{E}_{\text {cell }}^{\circ}}}\).
3 Applying an external opposite potential lower than \({\mathrm{\mathrm{E}_{\text {celll }}^{\circ}}}\)
4 Reversing the flow of ions in salt bridge.
JEE Main - 2024
CHXII03:ELECTROCHEMISTRY

330046 Assertion :
For the Daniell cell,
\(\mathrm{Zn}\left \vert \mathrm{Zn}^{2+}\right \vert \left \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}\) with \(\mathrm{E}_{\text {cell }}^{\mathrm{o}}=1.1 \mathrm{~V}\), the application of opposite potential greater than \({\text{1}}{\text{.1 V}}\) results into flow of electrons from cathode to anode.
Reason :
\(\mathrm{Zn}\) is deposited at anode and \(\mathrm{Cu}\) is dissolved at cathode.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
CHXII03:ELECTROCHEMISTRY

330047 In which of the following conditions salt bridge is not required in a galvanic cell?

1 When galvanic cell is used in geyser.
2 When distance between oxidation half cell and reduction half cell is negligible.
3 Electrolytic solution used in both the half cells are of same concentration.
4 When both the electrodes are dipped in the same electrolytic solution.
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CHXII03:ELECTROCHEMISTRY

330044 The electro-chemical cell stops working after some time because

1 Electrode potentials of both electrodes become zero
2 Electrode potentials of both electrodes become equal
3 Temperature of the cell increases
4 The reaction starts proceeding in opposite direction
CHXII03:ELECTROCHEMISTRY

330045 How can an electrochemical cell be converted into an electrolytic cell?

1 Exchanging the electrodes at anode and cathode.
2 Applying an external opposite potential greater than \({\mathrm{\mathrm{E}_{\text {cell }}^{\circ}}}\).
3 Applying an external opposite potential lower than \({\mathrm{\mathrm{E}_{\text {celll }}^{\circ}}}\)
4 Reversing the flow of ions in salt bridge.
JEE Main - 2024
CHXII03:ELECTROCHEMISTRY

330046 Assertion :
For the Daniell cell,
\(\mathrm{Zn}\left \vert \mathrm{Zn}^{2+}\right \vert \left \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}\) with \(\mathrm{E}_{\text {cell }}^{\mathrm{o}}=1.1 \mathrm{~V}\), the application of opposite potential greater than \({\text{1}}{\text{.1 V}}\) results into flow of electrons from cathode to anode.
Reason :
\(\mathrm{Zn}\) is deposited at anode and \(\mathrm{Cu}\) is dissolved at cathode.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
CHXII03:ELECTROCHEMISTRY

330047 In which of the following conditions salt bridge is not required in a galvanic cell?

1 When galvanic cell is used in geyser.
2 When distance between oxidation half cell and reduction half cell is negligible.
3 Electrolytic solution used in both the half cells are of same concentration.
4 When both the electrodes are dipped in the same electrolytic solution.
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CHXII03:ELECTROCHEMISTRY

330044 The electro-chemical cell stops working after some time because

1 Electrode potentials of both electrodes become zero
2 Electrode potentials of both electrodes become equal
3 Temperature of the cell increases
4 The reaction starts proceeding in opposite direction
CHXII03:ELECTROCHEMISTRY

330045 How can an electrochemical cell be converted into an electrolytic cell?

1 Exchanging the electrodes at anode and cathode.
2 Applying an external opposite potential greater than \({\mathrm{\mathrm{E}_{\text {cell }}^{\circ}}}\).
3 Applying an external opposite potential lower than \({\mathrm{\mathrm{E}_{\text {celll }}^{\circ}}}\)
4 Reversing the flow of ions in salt bridge.
JEE Main - 2024
CHXII03:ELECTROCHEMISTRY

330046 Assertion :
For the Daniell cell,
\(\mathrm{Zn}\left \vert \mathrm{Zn}^{2+}\right \vert \left \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}\) with \(\mathrm{E}_{\text {cell }}^{\mathrm{o}}=1.1 \mathrm{~V}\), the application of opposite potential greater than \({\text{1}}{\text{.1 V}}\) results into flow of electrons from cathode to anode.
Reason :
\(\mathrm{Zn}\) is deposited at anode and \(\mathrm{Cu}\) is dissolved at cathode.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
CHXII03:ELECTROCHEMISTRY

330047 In which of the following conditions salt bridge is not required in a galvanic cell?

1 When galvanic cell is used in geyser.
2 When distance between oxidation half cell and reduction half cell is negligible.
3 Electrolytic solution used in both the half cells are of same concentration.
4 When both the electrodes are dipped in the same electrolytic solution.
For More Updates join with Us
CHXII03:ELECTROCHEMISTRY

330044 The electro-chemical cell stops working after some time because

1 Electrode potentials of both electrodes become zero
2 Electrode potentials of both electrodes become equal
3 Temperature of the cell increases
4 The reaction starts proceeding in opposite direction
CHXII03:ELECTROCHEMISTRY

330045 How can an electrochemical cell be converted into an electrolytic cell?

1 Exchanging the electrodes at anode and cathode.
2 Applying an external opposite potential greater than \({\mathrm{\mathrm{E}_{\text {cell }}^{\circ}}}\).
3 Applying an external opposite potential lower than \({\mathrm{\mathrm{E}_{\text {celll }}^{\circ}}}\)
4 Reversing the flow of ions in salt bridge.
JEE Main - 2024
CHXII03:ELECTROCHEMISTRY

330046 Assertion :
For the Daniell cell,
\(\mathrm{Zn}\left \vert \mathrm{Zn}^{2+}\right \vert \left \vert \mathrm{Cu}^{2+}\right \vert \mathrm{Cu}\) with \(\mathrm{E}_{\text {cell }}^{\mathrm{o}}=1.1 \mathrm{~V}\), the application of opposite potential greater than \({\text{1}}{\text{.1 V}}\) results into flow of electrons from cathode to anode.
Reason :
\(\mathrm{Zn}\) is deposited at anode and \(\mathrm{Cu}\) is dissolved at cathode.

1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
CHXII03:ELECTROCHEMISTRY

330047 In which of the following conditions salt bridge is not required in a galvanic cell?

1 When galvanic cell is used in geyser.
2 When distance between oxidation half cell and reduction half cell is negligible.
3 Electrolytic solution used in both the half cells are of same concentration.
4 When both the electrodes are dipped in the same electrolytic solution.