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Given : Co^(3+) + e^(-) to Co^(2+) , E...

Given :
`Co^(3+) + e^(-) to Co^(2+)` , `E^(@) = +1.81V`
`pb^(4+) + 2e^(-) rightarrow Pb^(2+)` , `E^(@) = + 1.67V`
`Ce^(4)+ e^(-)rightarrow Ce^(3+), E^(@) = +1.61V`
`Ce^(4)+3e^(-)rightarrow Bi`, `E^(@) = + 0.20V`
Oxidation power of the species will increase in the order:

A

`Ce^(4+) ltPb^(4+) lt BI^(3+)ltCO^(3+)`

B

`CO^(3+)lt Ce^(4+)ltBi^(3+) lt Pb^(4+)`

C

`Bi^(3+lt Ce^(4+) ltPb^(4+) lt Co^(3+)

D

`CO^(3+)ltPb^(4+) lt Ce^(4+) lt Bi^(3+)`

Text Solution

AI Generated Solution

To determine the order of increasing oxidation power of the given species based on their reduction potentials, we can follow these steps: ### Step-by-Step Solution: 1. **Identify the Reduction Potentials**: We have the following half-reactions and their standard reduction potentials (E°): - \( \text{Co}^{3+} + e^- \rightarrow \text{Co}^{2+}, \quad E° = +1.81 \, \text{V} \) - \( \text{Pb}^{4+} + 2e^- \rightarrow \text{Pb}^{2+}, \quad E° = +1.67 \, \text{V} \) - \( \text{Ce}^{4+} + e^- \rightarrow \text{Ce}^{3+}, \quad E° = +1.61 \, \text{V} \) ...
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