InterviewSolution
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InterviewSolution
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Consider the following four electrodes: `A=Cu^(2+)(0.0001M)//Cu_((s))` `B=Cu^(2+)(0.1M)//Cu_((s))` `C= Cu^(2+)(0.01M)//Cu_((s))` `D=Cu^(2+)(0.001M)//Cu_((s))` If the standard reduction potential of `Cu^(+2)//Cu` is `+0.34V`, the reduction potentials (in volts) of the above electrodes follow the orderA. `PgtSgtRgtQ`B. `SgtRgtQgtP`C. `RgtgtRgtP`D. `QgtRgtSgtP` |
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Answer» Correct Answer - D `Cu^(2+)+2e ^(-)rarrCu` `E_("red")=E_("red")^(@)+(0.0591)/(2)"log"[Cu^(2+)]` `therefore` greater is `Cu^(2+)` ion concentration, greater will be the reduction potential. |
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