The standard voltage of the cell

Question

Pt I H2(g) I H (aq) II Cl- (aq) I AgCl (s) I Ag(s)

is .22 V at 25 deg C. Calculate the equilbrium constant for the reaction.

2 AgCl(s) H2(g) -> 2 Ag(s) 2H (aq) 2 Cl- (aq)

Answer 1

70 mv

Answer 2

yes ur rite!

Answer 3

first: hydrogen elecrode has 0Vstandard potential.this implies that

voltage of the cell E is equal to the Ag electrode potential AND IS

RELATED TO THE G OF THE HOLE RQN:2 AgCl(s) H2(g) -> 2 Ag(s) 2H (aq) 2 Cl- (aq)

second:G=-RTlnK ,G=-nFE ,lnK=FE/RT,K=exp(FE/RT)

K=exp(96500*0.22/8.31*298)=5287

K=5.287*10^3

third:u may go another route:in electrochemistry,for a mono-electronic

rqn,multipling by 10 modifies voltage by 0.059V

cell=0.220V >

0.220V/0.059V=3.723

K=10^(3.723)=5284 :) why is that?it has to do with the reaction quotient.