InterviewSolution
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InterviewSolution
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What is the correct nernst equation for reaction taking place in the following cell`Mg_((s))|Mg_((aq))^(2+)||Cl_((aq))^(-)|Cl_(2(g))(1atm)//Pt`A. `E_(cell)=E_(cell)^(o)-(0.0592)/(n)xxlog(([Cl^(-)]^(2))/([Mg^(2+)]))`B. `E_(cell)=E_(cell)^(o)-(0.0591)/(n)xxlog (([M^(2+)])/([Cl^(-)]))`C. `E_(cell)=E_(cell)^(@)-(0.592)/(n)xxlog[Mg^(2+)][Cl^(-)]^(2)`D. `E_(cell)=E_(cell)^(@)-(0.0591)/(n)xxlog(([Mg^(2+)])/([Cl^(-)]^(2)))` |
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Answer» Correct Answer - C `Mg_((s))|Mg_((aq))^(2+)||Cl_((aq))^(-)|Cl_(2(g))(1atm)//Pt` Oxidation half reaction, `MgtoMg^(2+)+2e^(-)` Reduction half reaction, `underline(Cl_(2)+2e^(-)to2Cl^(-)" ")` Net cell reaction, `Mg+Cl_(2)toMg^(2+)+2Cl^(-)` Nernst equation, `E_(cell)=E_(cell)^(o)-(0.0591)/(n)"log"[Cl^(-)]^(2)[Mg^(2+)]` Here, n=2 |
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