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  • Confused! kindly explain, - Redox Reaction and Electrochemistry - JEE Main-3

Given below are the half - cell reactions :

Mn^{2+} +2e^{-}\rightarrow Mn;E^{0}= -1.18 V

2\left ( Mn^{3+} +e^{-}\rightarrow Mn^{2+} \right );E^{0}= +1.51 V

The E^{0} for   3Mn^{2+} \rightarrow Mn+2Mn^{3+} will be :

  • Option 1)

     -2.69 V ; the reaction will not occur
     

  • Option 2)

     -2.69 V ; the reaction will occur

  • Option 3)

     -0.33 V ; the reaction will not occur

     

  • Option 4)

    -0.33 V ; the reaction will occur

 

Answers (1)

best_answer

As we have learned

M(s) is Solid -

[M] = 1

- wherein

E_{M^{n+}/M}=E_{M^{n+}/M}^{0}-\frac{RT}{nf}ln\frac{1}{[M^{n+}]}

 

 

 

 Mn^{2+} +2e^-\rightarrow Mn \; \; \; \; \; E^0 = -1.18V

2Mn^{2+} \rightarrow 2Mn^{3+}+2e^- \; \; \; \; \; E^0 = -1.51V

______________________________

3Mn^{2+} \rightarrow Mn+2Mn^{3+} \; \; \; \; \; E^0 = SOP +SRP

 

E_{Mn^{2+}/Mn^{3+}}^{0}= -1.18 + (-1.51 )= -2 .69 V

Negative EMF raflects non spaontaneous cell raection 

\Delta G = - nFE_{cell}

 

 

 

 


Option 1)

 -2.69 V ; the reaction will not occur
 

Option 2)

 -2.69 V ; the reaction will occur

Option 3)

 -0.33 V ; the reaction will not occur

 

Option 4)

-0.33 V ; the reaction will occur

Posted by

SudhirSol

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