. Calculate E°cell and ∆rG° for the following reaction at 25°C. A2+(aq) + B+(aq) → A3+(aq) + B(s) [Given KC = 1010, 1F = 96500 C, R = 8.314 JK–1 mol–1]

Q. Calculate the equilibrium constant for the following reaction:
$Cu\left(s\right)+2{Ag}^{+}(aq.)\rightleftharpoons {Cu}^{2+}\left(aq\right)+2Ag\left(s\right)$
At ${25}^{o}C$, $E_{cell}^o=0.47volt,R=8.314J{K}^{-1}{mol}^{-1},F=96500coulomb$

Q. (a) The cell in which the following reaction occurs:
$2F{e}^{3+}\left(aq\right)+2I^{-}\left(aq\right)\to 2F{e}^{2+}\left(aq\right)+I_2\left(s\right)$ has $E_{\text{cell}}^{⊝}=0.236V$ at 298 K.
Calculate the standard Gibbs energy of the cell reaction. (Given: 2F= 96500 C $mo{l}^{-1}$)
(b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F= 96500 C $mo{l}^{-1}$)

Q. a) Draw labelled diagram of Standard Hydrogen Electrode ( SHE ).
Write its half cell reaction of $E^o$ value.
b) Calculate $△r{G}^{⊝}$ for the following reaction :
$F{e}_{\left(aq\right)}^{+2}+A{g}_{\left(aq\right)}^{+}\to {Fe}_{\left(aq\right)}^{+3}+A{g}_{\left(s\right)}$.
(Given : $E_{Cell}^0=+0.03V,F=96500C$).

Q. (a) The cell in which the following reaction occurs:
$2F{e}^{3+}\left(aq\right)+2I^{-}\left(aq\right)\to 2F{e}^{2+}\left(aq\right)+I_2\left(s\right)$ has $E_{\text{cell}}^{⊝}=0.236V$ at 298 K.
Calculate the standard Gibbs energy of the cell reaction. (Given: 2F= 96500 C $mo{l}^{-1}$)
(b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F= 96500 C $mo{l}^{-1}$)