Consider the following E^{\circ} values.

E^{\circ}{_{Fe^{3+}/Fe^{2+}}}= +0.77V,E^{\circ}{_{Sn^{2+}/Sn}}= -0.14V

Under standard conditions the potential for the reaction

Sn_{(s)}+2Fe^{3+}{_{\left ( aq \right )}}\rightarrow 2Fe^{2+}{_{\left ( aq \right )}}+Sn^{2+}{_{\left ( aq \right )}} is

 

 

  • Option 1)

    1.68 V

  • Option 2)

    1.40 V

  • Option 3)

    0.91 V

  • Option 4)

    0.63 V.

 

Answers (1)

As we learnt in

Standard Electrode Potential -

If concentration of each species taking part in the electrode reaction is unity and further the reaction is carried out at 298 K, then the potential of each electrode is said to be the standard electrode potential.

-

 

and

Electrode Potential -

The potential associated with each electrode is known as electrode potential.

-

 

  

E^{\circ}_{cell}=E^{\circ}_{Sn/Sn^{2+}}+E^{\circ}_{Fe^{3+}/Fe^{2+}}

=0.14+0.77=0.91\, V


Option 1)

1.68 V

This option is incorrect.

Option 2)

1.40 V

This option is incorrect.

Option 3)

0.91 V

This option is correct.

Option 4)

0.63 V.

This option is incorrect.

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