InterviewSolution
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InterviewSolution
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Redox reactions play a pivotal role in chemistry and biology. The values of standard redox potential `(E^(@))` of two half-cell reactions decide which way the reaction is expected to proceed. A simple example is a Daniel cell in which zinc goes into solution and copper gets deposited. `E^(@)(SRP)` of different half cells are given below: `E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V` `E_(Ag^(+)|Ag=0.8V, E_(Mg^(2+)|Mg))=-2.37V` In which cell, `DeltaG^(@)` per "mole" of electron is most negative?A. `Zn(s)|Zn^(2+)(1M)||Mg^(2+)(1M)|Mg(s)`B. `Zn(s)|Zn^(2+)(1M)||Ag^(+)(1M)|Ag(s)`C. `Cu(s)|Cu^(2+)(1M)||Ag^(+)(1M)|Ag(s)`D. `Ag(s)|Ag^(+)(1M)||Mg^(2+)(1M)|Mg(s)` |
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Answer» Correct Answer - B |
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