Electrochemical Cells, Galvanic Cells
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How can chemical energy be converted into electrical energy?
Explain Daniel cell with cell diagram representation and process taking place in the cell.
- Zn rod in CuSO4 solution
- Zn rod in ZnSO4 solution
- Cu rod in ZnSO4 solution
- Cu rod in CuSO4 solution
- the velocity of K+ is greater than that of NO−3
- the velocity of K+ is lesser than that of NO−3
- the velocity of K+ and NO−3 are nearly the same
- KNO3 is highly soluble in water
The nature of electolytes used in a salt bridge are:
Inert electrolytes
Any electrolyte can be used
Weak electrolytes
Non electrolytes
Which of the following is FALSE regarding the salt bridge used in voltaic cells? The salt bridge:
allows two half-cells to be separated
maintains electrical neutrality in half cells
allows mixing of the two electrode solutions
allows ions to cross over slowly
Cathode : graphite
- cathode : iron
Anode : graphite
- Anode : iron
Assertion : Salts like KCl, KNO3 i.e., inert electrolytes are used in salt bridge.
Reason : An inert electrolyte can easily be filled in the U-tube.
- If both assertion and reason are true and the reason is the correct explanation of the assertion.
- If both assertion and reason are true but reason is not the correct explanation of the assertion.
- If assertion is true but reason is false.
- If the assertion and reason both are false.
- A fuel cell
- An electrolytic cell
- A galvanic cell
- A concentration cell
- Cu(s)→Cu2+(aq)+2e−
- Cu2+(aq)+2e−→Cu(s)
- Zn(s)→Zn2+(aq)+2e−
- Zn2+(aq)+2e−→Zn(s)
- Electrons flow from copper electrode to zinc electrode
- Current flows from zinc electrode to copper electrode
- Cations move towards copper electrode
- Anions move towards copper electrode
- Non-spontaneous reaction will occur
- Electrons flow is opposite to galvanic cell
- Both (b) and (c)
- Spontaneous reaction will occur
- Electrode potential of both the electrodes becomes zero
- Electrode potential of both the electrodes becomes equal
- The reaction starts proceeding in opposite direction
- None of these
MnO−4+8H++5e−→Mn+2+4H2O,
Eo=1.51 V.
The quantity of electricity required in Faraday to reduced five moles of MnO−4 is
(Integer answer)
( <!--td {border: 1px solid #ccc;}br {mso-data-placement:same-cell;}--> JEE MAIN 2021)
Using the standard electrode potentials given in the Table 8.1, predict if the reaction between the following is feasible:
(a) Fe3+(aq) and I–(aq)
(b) Ag+(aq) and Cu(s)
(c) Fe3+ (aq) and Cu(s)
(d) Ag(s) and Fe3+(aq)
(e) Br2(aq) and Fe2+(aq)