The equilibrium constant at 298 K for the reaction Cu(s) + 2Ag+ (aq) ⇌ Cu2+ (aq) + 2Ag(s) is 2.0 × 1015 . The concentrations of Cu2+ and Ag+ ions are 1.8 × 10-2 mol L-1 and 3.0 x 10-19 mol L-1 respectively. Is this reaction at equilibrium?

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

The equilibrium constant for the reaction, Ag_2O(s) hArr2Ag(s) +1/2 O_2 (g) is given by

The equilibrium constant for a cell reaction, Cu(g) + 2Ag^+(aq) → Cu^(2+)(aq) + 2Ag (s) is 4 × 10^16 . Find E° (cell) for the cell reaction.

The equilibrium constant at 278 K for Cu(s) +2Ag ^(+) (aq) hArr Cu^(2+) (aq) + 2Ag(s) is 2.0 xx 10^(15) . At a particular moment , the concentration of Cu^(2+) and Ag^(+) ions are found to be 1.8 xx 10 ^(-2) " mol " L^(-1) and 3.0 xx 10 ^(-9) " mol " L^(-1) respectively . Is the system in equilibrium at that moment?

The equilibrium constant of the reaction : Zn(s)+2Ag^(+)(aq)toZn(aq)+2Ag(s),E^(@)=1.50V at 298 K is

Calculate the equilibrium constant of the reaction : Cu(s)+2Ag(aq) hArrCu^(2+)(aq) +2Ag(s) E^(c-)._(cell)=0.46V

Calculate the equilibrium constant of the reaction : Cu(s)+2Ag(aq) hArrCu^(2+)(aq) +2Ag(s) E^(c-)._(cell)=0.46V

Write the equilibrium constant expressions for the following reactions. Cu( s)+ 2Ag^(+) (aq) hArr Cu^(2+) (aq) + 2Ag(s)

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