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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

AI Generated Solution

The correct Answer is:
To solve the problem, we need to analyze the given standard reduction potentials (E°) for the redox couples and determine which species can be reduced by another based on their oxidizing and reducing abilities. ### Step-by-Step Solution: 1. **List the Given E° Values**: - \( \text{Br}_2/\text{Br}^- = +1.90 \) - \( \text{Ag}^+/\text{Ag(s)} = +0.80 \) - \( \text{Cu}^{2+}/\text{Cu(s)} = +0.34 \) - \( \text{I}_2/\text{I}^- = +0.54 \) 2. **Understand the Concept of Reduction Potential**: - The higher the E° value, the stronger the oxidizing agent. Conversely, the lower the E° value, the stronger the reducing agent. 3. **Rank the Redox Couples by E° Values**: - From highest to lowest: 1. \( \text{Br}_2/\text{Br}^- = +1.90 \) (strongest oxidizing agent) 2. \( \text{Ag}^+/\text{Ag(s)} = +0.80 \) 3. \( \text{I}_2/\text{I}^- = +0.54 \) 4. \( \text{Cu}^{2+}/\text{Cu(s)} = +0.34 \) (weakest oxidizing agent) 4. **Determine Which Species Can Be Reduced**: - Since \( \text{Br}_2 \) has the highest E° value, it will be reduced first by any suitable reducing agent. - The reducing agents in this case are \( \text{Cu} \), \( \text{Ag} \), and \( \text{I}^- \). 5. **Identify the Correct Reducing Reaction**: - Among the options given: - \( \text{Cu} \) can reduce \( \text{Br}_2 \) because \( \text{Cu} \) has a lower E° value than \( \text{Br}_2 \). - \( \text{Cu} \) cannot reduce \( \text{Ag}^+ \) because \( \text{Ag}^+ \) has a higher E° value than \( \text{Cu}^{2+} \). - \( \text{Cu} \) cannot reduce \( \text{I}_2 \) because \( \text{I}_2 \) has a higher E° value than \( \text{Cu}^{2+} \). - \( \text{Cu} \) cannot reduce \( \text{Br}^- \) because \( \text{Br}^- \) is already in its reduced form. 6. **Conclusion**: - The only correct option is that \( \text{Cu} \) will reduce \( \text{Br}_2 \). ### Final Answer: **D. \( \text{Cu} \) will reduce \( \text{Br}_2 \)**.
To solve the problem, we need to analyze the given standard reduction potentials (E°) for the redox couples and determine which species can be reduced by another based on their oxidizing and reducing abilities. ### Step-by-Step Solution: 1. **List the Given E° Values**: - \( \text{Br}_2/\text{Br}^- = +1.90 \) - \( \text{Ag}^+/\text{Ag(s)} = +0.80 \) - \( \text{Cu}^{2+}/\text{Cu(s)} = +0.34 \) ...
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