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E^(θ) values of some redox couples are g...

`E^(θ)` values of some redox couples are given below. On the basis of these values choose the correct option.
`E^(θ)` values: `Brt_(2)//Br^(-) = +1.90`
`Ag^(+)//Ag(s)=+0.80`
`Cu^(2+)//Cu(s)=+0.34, I_(2)(s)//I^(-)=+0.54`

A

Cu will reduce `Br^(-)`

B

Cu will reduce Ag

C

Cu will reduce `I^(-)`

D

Cu will reduce `Br_(2)`

Text Solution

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The correct Answer is:
To solve the given problem, we will analyze the provided standard reduction potentials (E° values) for the redox couples and determine the correct option based on their oxidizing and reducing abilities. ### Step-by-Step Solution: 1. **List the Given Standard Reduction Potentials**: - \( \text{Br}_2/\text{Br}^- = +1.90 \, \text{V} \) - \( \text{Ag}^+/\text{Ag}(s) = +0.80 \, \text{V} \) - \( \text{Cu}^{2+}/\text{Cu}(s) = +0.34 \, \text{V} \) - \( \text{I}_2(s)/\text{I}^- = +0.54 \, \text{V} \) 2. **Determine the Order of Reduction Potentials**: - The higher the E° value, the stronger the oxidizing agent. Thus, we can arrange the couples in decreasing order of their reduction potentials: - \( \text{Br}_2 > \text{Ag}^+ > \text{I}_2 > \text{Cu}^{2+} \) - This means: - \( \text{Br}_2 \) is the strongest oxidizing agent. - \( \text{Cu}^{2+} \) is the weakest oxidizing agent. 3. **Analyze the Reducing Ability**: - A species with a lower E° value can act as a reducing agent for a species with a higher E° value. Therefore: - \( \text{Cu} \) can reduce \( \text{Br}_2 \), \( \text{Ag}^+ \), and \( \text{I}_2 \) but cannot reduce \( \text{Br}^- \) because \( \text{Br}^- \) is already reduced. - \( \text{Cu} \) cannot reduce \( \text{Ag} \) because \( \text{Ag}^+ \) is already at a higher potential. 4. **Evaluate Each Option**: - **Option A**: \( \text{Cu} \) will reduce \( \text{Br}^- \) - **Incorrect**. \( \text{Br}^- \) is already reduced. - **Option B**: \( \text{Cu} \) will reduce \( \text{Ag} \) - **Incorrect**. \( \text{Cu} \) cannot reduce \( \text{Ag}^+ \) as it is a stronger oxidizing agent. - **Option C**: \( \text{Cu} \) will reduce \( \text{I}^- \) - **Incorrect**. \( \text{Cu} \) cannot reduce \( \text{I}^- \) as it is already reduced. - **Option D**: \( \text{Cu} \) will reduce \( \text{Br}_2 \) - **Correct**. \( \text{Cu} \) can reduce \( \text{Br}_2 \) to \( \text{Br}^- \). 5. **Conclusion**: - The correct option is **D**: \( \text{Cu} \) will reduce \( \text{Br}_2 \).
To solve the given problem, we will analyze the provided standard reduction potentials (E° values) for the redox couples and determine the correct option based on their oxidizing and reducing abilities. ### Step-by-Step Solution: 1. **List the Given Standard Reduction Potentials**: - \( \text{Br}_2/\text{Br}^- = +1.90 \, \text{V} \) - \( \text{Ag}^+/\text{Ag}(s) = +0.80 \, \text{V} \) - \( \text{Cu}^{2+}/\text{Cu}(s) = +0.34 \, \text{V} \) ...
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