Every question from past board papers on Cell potential and Gibbs energy, newest paper first. Open any question for its full worked answer.
Given below are two statements : one is labelled as Assertion A and the other is labelled as Reason R :
Assertion A : In equation \(\Delta_r G = -nFE_{cell}\), value of \(\Delta_r G\) depends on n.
Reasons R : \(E_{cell}\) is an intensive property and \(\Delta_r G\) is an extensive property.
In the light of the above statements, choose the correct answer from the options given below :
For the cell reaction
\(2Fe^{3+}(aq) + 2I^{-}(aq) \to 2Fe^{2+}(aq) + I_2(aq)\)
\(E^{\ominus}_{cell} = 0.24\) V at 298 K. The standard Gibbs energy (\(\Delta_rG^{\ominus}\)) of the cell reaction is :
[Given that Faraday constant F = 96500 C mol\(^{-1}\)]
For a cell involving one electron \(E^{\ominus}_{cell} = 0.59\) V at 298 K, the equilibrium constant for the cell reaction is :
[Given that \(\frac{2.303\,RT}{F} = 0.059\) V at T = 298 K]
If the \(E^\circ_{cell}\) for a given reaction has a negative value, which of the following gives the correct relationships for the values of \(\Delta G^\circ\) and \(K_{eq}\)?
