The equilbrium constant for the reaction : `Cu + 2 Ag^(+) (aq) rarr Cu(2+) (aq) +2 Ag, E^@ = 0. 46 V` at ` 299 K` is

The equivalent constant of the reaction: Cu(s)+2Ag^(+)(aq.) rarr Cu^(2+)(aq.)+2Ag(s) E^(@)=0.46 V at 298 K ,is:

The equilibrium constent of the reaction. Cu(s)+2Ag(aq). Leftrightarrow Cu^(2+) (aq.)+2Ag(s) E^(@)=0.46" V at 298 K is"

The equilibrium constant for the reaction Cu_(s) + 2Ag^+ _ (aq) rarr Cu^2+ _ (aq) +2Ag at 298 k is Given E^@cell=0.46v

The equilibrium constant for the reactions Cu (s)+ 2Ag^(+) aq hArr Cu^(2+) (aq) +2Ag(s) is 2.0 xx 10 ^(15) " at " 278 K. Find the equilibrium concentration of Cu^(2+) (aq) if that of Ag^(+) (aq) is 1.0 xx 10 ^(-11) " mol " L^(-1)

The equilibrium constant of the reaction; Cu(s)+2Ag + (aq)⟶Cu 2+ (aq)+2Ag(s) E o =0.46V at 298K

Calculate the equilibrium constant of the reaction: Cu(s) + 2Ag^+(aq) → Cu^(2+) (aq) + 2Ag(s) E^o(cell) = 0.46 V

Calculate the equilibrium constant of the reaction: Cu_(s)+2Ag_(aq)^(+) rarr Cu_(aq)^(2+) + 2Ag_(s) , E_^@cell_^@ = 0.46V .

Calculate the equilibrium constant of the reaction : Cu(s)+2Ag^(+)(aq)rarr Cu^(2+)(aq)+2Ag(s): E_("cell")^(@)=0.46V