Calculate the reduction potential of a half cell consisting of a platinum electrode immersed in `2.0M Fe^(2+)` and `0.02M Fe^(3+)` solution. Given `E_(Fe^(3+)//Fe^(2+))^(@) = 0.771 V`.

Calculate the reduction potential of a half cell consisting of a plati

1.	Calculate the reduction potential of a half cell consisting of a platinum electrode immersed in `2.0M Fe^(2+)` and `0.02M Fe^(3+)` solution. Given `E_(Fe^(3+)//Fe^(2+))^(@) = 0.771 V`.
Answer» The half cell reaction is : `Fe^(3+)+e rarr Fe^(2+)` (or take `Fe^(2+) rarr Fe^(3+)+e`) Thus `E_(Fe^(3+)//Fe^(2+)) = E_(Fe^(3+)//Fe^(2+))^(@) + (0.059)/(1)"log"([Fe^(3+)])/ ([Fe^(2+)])` `:. E_(Fe^(3+)//Fe^(2+)) = 0.771 + (0.059)/(1)"log"(0.02)/(2.0)` `= 0.771 +(0.059)/(1)"log"10^(-2) = 0.653 V`

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Calculate the reduction potential of a half cell consisting of a platinum electrode immersed in `2.0M Fe^(2+)` and `0.02M Fe^(3+)` solution. Given `E_(Fe^(3+)//Fe^(2+))^(@) = 0.771 V`.

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