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The more positive the value of E^(θ), th...

The more positive the value of `E^(θ)`, the greater is the trendency of the species to get reduced. Using the standard electrode potential of redox coples given below find out which of the following is the strongest oxidising agent.
`E^(θ)` values: `Fe^(3+)//Fe^(2+) = +0.77`
`I_(2)(s)//I^(-) = +0.54`,
`Cu^(2+)//Cu = +0.34, Ag^(+)//Ag = 0.80V`

A

`Fe^(3+)`

B

`I_(2(s))`

C

`Cu^(2+)`

D

'Ag^(+)'

Text Solution

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The correct Answer is:
To determine which of the given species is the strongest oxidizing agent based on their standard electrode potentials, we will follow these steps: ### Step 1: Understand the Concept of Standard Electrode Potential The standard electrode potential (E°) indicates the tendency of a species to gain electrons and be reduced. A more positive E° value means a greater tendency to be reduced, and thus, a stronger oxidizing agent. ### Step 2: List the Given Standard Electrode Potentials We have the following standard electrode potentials for the redox couples: - \( \text{Fe}^{3+}/\text{Fe}^{2+} = +0.77 \, \text{V} \) - \( \text{I}_2(s)/\text{I}^- = +0.54 \, \text{V} \) - \( \text{Cu}^{2+}/\text{Cu} = +0.34 \, \text{V} \) - \( \text{Ag}^+/ \text{Ag} = +0.80 \, \text{V} \) ### Step 3: Compare the E° Values Now, we will arrange the given E° values in descending order to identify which species has the highest potential: 1. \( \text{Ag}^+/\text{Ag} = +0.80 \, \text{V} \) (highest) 2. \( \text{Fe}^{3+}/\text{Fe}^{2+} = +0.77 \, \text{V} \) 3. \( \text{I}_2(s)/\text{I}^- = +0.54 \, \text{V} \) 4. \( \text{Cu}^{2+}/\text{Cu} = +0.34 \, \text{V} \) (lowest) ### Step 4: Identify the Strongest Oxidizing Agent From the above arrangement, we can see that \( \text{Ag}^+ \) has the highest standard electrode potential of +0.80 V. Therefore, \( \text{Ag}^+ \) is the strongest oxidizing agent among the given options. ### Conclusion The strongest oxidizing agent is \( \text{Ag}^+ \). ---
To determine which of the given species is the strongest oxidizing agent based on their standard electrode potentials, we will follow these steps: ### Step 1: Understand the Concept of Standard Electrode Potential The standard electrode potential (E°) indicates the tendency of a species to gain electrons and be reduced. A more positive E° value means a greater tendency to be reduced, and thus, a stronger oxidizing agent. ### Step 2: List the Given Standard Electrode Potentials We have the following standard electrode potentials for the redox couples: - \( \text{Fe}^{3+}/\text{Fe}^{2+} = +0.77 \, \text{V} \) ...
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