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Derive an equation for equilibrium constant K_(c) of any galvanic cell (Redox reaction) and also give its uses. |
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Answer» Solution :* According to the active mass rule when any redox reaction attains equilibrium then, * At equilibrium both electrode potential becomes zero, `E_(CELL)=0.0V` and so its nernst equation will be as follows: `0.0=E_(cell)=E_(cell)^(Theta)-(0.059)/(n)logQ` `therefore E_(cell)^(Theta)-(0.059)/(n)logK_(C)""(logQ=logK_(C))` `therefore logK_(C)=(nxxE^(Theta))/(0.059)` `therefore K_(C)="Antilog "(n E^(Theta))/(0.059)` Where, n= number of electrons differ in the reaction `E^(Theta)=`standard reduction potential of redox reaction `=E_("cathode")^(Theta)-E_("anode")^(Theta)` * Uses : (i) equilibrium CONSTANT can be calculated by MEASURING potential. (ii) value of `K_(C)` gives account of reaction. if `K_(C)` value is hihgh then FORWARD reaction will be more and so more product will be obtained. |
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