Zinc can be coated on iron to produce galvanized iron,but the reverse is not possible. This is because:
- Azinc is lighter than iron
- Bzinc has a lower melting point than iron
- Czinc has a lower negative electrode potential than iron
- Dzinc has a higher negative electrode potential than iron
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$K,$ $Ca,$ and $Li$ metals may be arranged in the increasing order of their standard electrode potentials as
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View SolutionTwo half-cell reactions are given below:
$Co^{3+} + e^- \rightarrow Co^{2+}, E^{\circ}_{Co^{3+}/Co^{2+}} = 1.81 \, V$
$Al^{3+} + 3e^- \rightarrow Al(s), E^{\circ}_{Al^{3+}/Al} = -1.66 \, V$
The standard $EMF$ of a cell with a feasible redox reaction will be:
$Co^{3+} + e^- \rightarrow Co^{2+}, E^{\circ}_{Co^{3+}/Co^{2+}} = 1.81 \, V$
$Al^{3+} + 3e^- \rightarrow Al(s), E^{\circ}_{Al^{3+}/Al} = -1.66 \, V$
The standard $EMF$ of a cell with a feasible redox reaction will be:
MediumNEET 2022
View SolutionGiven $E_{Cu^{2+}/Cu}^{\circ} = 0.34 \ V$ and $E_{Cu^{2+}/Cu^{+}}^{\circ} = 0.15 \ V$. Calculate the standard electrode potential $E_{Cu^{+}/Cu}^{\circ}$ in $V$.
Medium
View SolutionWhich of the following reactions will be spontaneous in an electrochemical cell constructed from the given standard electrode potentials: $E_{Cl_2 \mid 2Cl^-}^0 = 1.36 \ V$ and $E_{Br_2 \mid 2Br^-}^0 = 1.09 \ V$?
Which of the following relations about $E^{\circ}_{cell}$ is false?
DifficultMHT CET 2025
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