The standard electrode potentials of the electrodes are given below. Arrange them in decreasing order of ease of oxidation. (1) Electrode \(-\mathrm{I}, \mathrm{E}^{\circ}=-2.89 \mathrm{~V}\) (2) Electrode - II, E \(^{\circ}=-0.16 \mathrm{~V}\) (3) Electrode \(-\mathrm{III}, \mathrm{E}^{\circ}=0.77 \mathrm{~V}\) (4) Electrode \(-\mathrm{IV}, \mathrm{E}^{\circ}=-2.93 \mathrm{~V}\) (5) Electrode \(-\mathrm{V}, \mathrm{E}^{\circ}=-1.67 \mathrm{~V}\) (a) 32514 (b) 41523 (c) 35142 (d) 32145

Question: Arrange the given electrodes in decreasing order of ease of oxidation. Options: a) 12345 b) 41523 c) 23154 d) 52413 Given standard electrode potentials: 1. Electrode I: \(E^{\circ}=-2.89V\) 2. Electrode II: \(E^{\circ}=-0.16V\) 3. Electrode III: \(E^{\circ}=0.77V\) 4. Electrode IV: \(E^{\circ}=-2.93V\) 5. Electrode V: \(E^{\circ}=-1.67V\) We know that the lower (more negative) the standard electrode potential is, the easier it is for a substance to be oxidized. Sorting the given electrode potential values in increasing order, we get: 1. Electrode IV: \(-2.93V\) 2. Electrode I: \(-2.89V\) 3. Electrode V: \(-1.67V\) 4. Electrode II: \(-0.16V\) 5. Electrode III: \(0.77V\) This order matches with option (b). Answer: (b) 41523