Now, calculate the cell voltage using the given half-reactions. The solubility products (KD) for AgCl and...

Question

Question

Answer 1

Answer #1

For CuI,

CuI => Cu+ + I-

Ksp= [Cu+] [I-]

E1= E0 - (0.0592/n) log ([Cu+][I-])

=0.518 - (0.0592).log(Ksp) => 0.518 - (0.0592) log (1.0* 10-12)

E1 = 1.228 V

For AgCl,

AgCl => Ag+ + Cl-

Ksp= [Ag+] [Cl-]

E2= E0 - (0.0592/n) log ([Ag+][Cl-])

=0.7993 - (0.0592).log(Ksp) => 0.7993 - (0.0592) log (1.8* 10-10)

E2 = 1.376 V

Cell potential for ; Cu + Ag+ => Cu+ + Ag

Ecell= E2 - E1 = 1.376 - 1.228

Ecell= 0.148 V

Answer 2

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