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InterviewSolution
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For the electrochemical cell, `Mg(s)|Mg^(2+) (aq. 1M)||Cu^(2+) (aq. 1M)|Cu(s)` the standard emf of the cell is 2.70 V at 300 K. When the concentration of `Mg^(2+)` is chaged to x M, the cell potential changes to 2.67 V at 300 K. The value of x is ________ . (Given `F/R=11500 kV^(-1)`. where F is the Faraday constant and R is the gas constant, ln (10) = 2.30) |
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Answer» Correct Answer - 10 Cell reaction : `Mg(s)+Cu^(2+) (aq) hArr Mg^(2+) (aq)+Cu(s)" "(n=2)` when the concentration of ionic species is 1 M then `E=E^(@)` `:. E^(@)=2.70 V` Using Nernst equation : `E=E^(@)-(RT)/(nF)"ln" ([Mg^(2+)])/([Cu^(2+)])` `2.67=2.70-(RT)/(2F) log_(e) [x/1]` `ln x=(0.03xx2)/300xxF/R=(0.03xx2xx11500)/(300)` `=2.30=ln 10` `x=10` |
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