The standard emf of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at $25^{o} C$ . The equilibrium constant of the reaction would be
(Given, $F = 96500 C m o l^{- 1}, R = 8. 314 J K^{- 1} m o l^{- 1}$ )

Question

The standard emf of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at

25^{o} C

. The equilibrium constant of the reaction would be
(Given,

F = 96500 C m o l^{- 1}, R = 8. 314 J K^{- 1} m o l^{- 1}

)

Toppr Admin · Accepted Answer

For a cell reaction in equilibrium at 298 KEoCell-0-0591nlogKc-x21D2-logKc-Eocell-xD7-n0-0591Substitute the given values of Eocell and n in the above equation- we get

The standard emf of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25oC. The equilibrium constant of the reaction would be(Given, F=96500Cmol−1,R=8.314JK−1mol−1 )2.0×10114×10121×1021×1010

For a cell reaction in equilibrium at 298 KEoCell=0.0591nlogKc⇒logKc=Eocell×n0.0591Substitute the given values of Eocell and n in the above equation, we get

For a cell reaction in equilibrium at 298 K

$E_{C e l l}^{o} = \frac{0.0591}{n} l o g K_{c}$

$\Rightarrow l o g K_{c} = \frac{E_{c e l l}^{o} \times n}{0.0591}$

Substitute the given values of $E_{c e l l}^{o}$ and n in the above equation, we get