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At equimolar concentration of `Fe^(2+)` and `Fe^(3+)`, what must `[Ag^(+)]` be so that the voltage of the galvanic cell made from the `(Ag^(+) | Ag)` and `(Fe^(3+)|Fe^(2+)` electrodes equals zero? `Fe^(2+) + Ag^(+) rightarrow Fe^(3+) + Ag` `E_(Ag^(+), Ag)^(@)`= 0.7991, `E_(Fe^(3+)//Fe^(2+))^(@) = 0.771`A. 0.34B. 0.44C. 0.47D. 0.61 |
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Answer» Correct Answer - A `0=(0.771+0.7991)-(0.0591)/(1)log((1)/(x))implies0=0.0281+0.051logX` `logX=-(0.0281)/(0.0591)impliesX=0.335M` |
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