The standard free energy change for the given reaction is - 10.26 kcal mol−1 at 25∘C.H2(g)+2AgCl(s)→2Ag(s)+2H+(aq)+2Cl−(aq)A cell using the above reaction is operated at 25∘C under conditions,PH2=1 atm[H+] and [Cl−]=0.1 MCalculate the emf of the cell.(Up to two decimal ,where 2.303RTF=0.059,R=8.314 J K−1,F=96500C)

The standard free energy change for the given reaction is - 10.26 kcal

1.	The standard free energy change for the given reaction is - 10.26 kcal mol−1 at 25∘C.H2(g)+2AgCl(s)→2Ag(s)+2H+(aq)+2Cl−(aq)A cell using the above reaction is operated at 25∘C under conditions,PH2=1 atm[H+] and [Cl−]=0.1 MCalculate the emf of the cell.(Up to two decimal ,where 2.303RTF=0.059,R=8.314 J K−1,F=96500C)
Answer» The standard free energy change for the given reaction is - $10.26 k c a l m o l^{- 1}$ at $25^{\circ} C .$ $H_{2} (g) + 2 A g C l (s) \to 2 A g (s) + 2 H^{+} (a q) + 2 C l^{-} (a q)$ A cell using the above reaction is operated at $25^{\circ} C$ under conditions, $P_{H_{2}} = 1 a t m$ $[H^{+}] and [C l^{-}] = 0.1 M$ Calculate the emf of the cell. (Up to two decimal ,where $\frac{2.303 R T}{F} = 0.059, R = 8.314 J K^{- 1}, F = 96500 C$ )