Given that E0Cl2/Cl−=1.35V and Ksp(AgCl)=10−10 at 25oC.
E0 corresponding to the electrode reaction is 12Cl2(g)+Ag+(aq)+e−→AgCl(s) is
A
0.75V
No worries! We‘ve got your back. Try BYJU‘S free classes today!
B
1.05V
No worries! We‘ve got your back. Try BYJU‘S free classes today!
C
2.65V
No worries! We‘ve got your back. Try BYJU‘S free classes today!
D
1.94V
Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses
Open in App
Solution
The correct option is D1.94V For sparingly soluble AgCl AgCl(s)→Ag+(aq)+Cl−(aq)...(eq1) Ksp(AgCl)=10−10 ΔG1=−RTlnKsp
For : 12Cl2(g)+e−→Cl−(aq)......(eq2);E02=1.35V ΔG2=−nFE02
Reversing eqn 1 and adding with equation 2, we get the desired equation 12Cl2(g)+Ag+(aq)+e−→AgCl(s)...(eq3) ΔG3=−nFE03=ΔG2−ΔG1 −nFE03=−nFE02−(−RTlnKsp) E03=E02−RTFln10−10E03=1.35+(0.059×10)=1.94V