For the disproportionation reaction `2Cu^(+)(aq)hArrCu(s)+Cu^(2+)(aq)` at K, In K (where K is the equilibrium constant) is ________ `xx10^(–1)`.
Given : `( E_(Cu^(2+)//Cu^+)^@ = 0.16V and E_(Cu^(+)//Cu)^@ = 0.52V)`

The standard emf for the cell reaction, 2Cu^(+)(aq)to2Cu(s)+Cu^(2+)(aq) is 0.36V at 298K . The equilibrium constant of the reaction is

E_(Cu^(2+)//Cu)^(@)=0.34V E_(Cu^(+)//Cu)^(@)=0.522V E_(Cu^(2+)//Cu^(+))^(@)=

for cell reaction 2Cu^+ rarr Cu +Cu^(2+) Find lnK = ......xx10^(-1) where K is equlibrium constant. given Cu^+ + e^- rarr Cu E^@ = 0.52 Cu

The standard e.m.f. for the cell reaction. 2Cu^(+)(aq)rarrCu(s)+Cu^(2+)(aq) is +0.36 V at 298K. The equilibrium constant of the reaction is

For the reaction: Cu(s) + 2Ag_((aq))^+ Leftrightarrow Cu_((aq))^(2+) +2Ag_((s)) , the equilibrium constant is given by

Calculate equilibrium constant for tha disproportionation reaction : 2Cu^(2+)(aq)rarrCu(s)+Cu^(2+)(aq)" at " 25^(@)C ("Given " E_((Cu^(+)//Cu))^(@)=0.52 V, E_((Cu^(2+)//Cu^(+)))^(@)=0.16 V) .

Cu^(2+)(aq.) is unstable in solution and under goes simultaneous oxidation and reduction according to the reaction 2Cu^(+)(aq.)hArr Cu^(2+)(aq.)+Cu(s) Choose the correct E^(@) for the above reaction if E_(Cu^(2+))^(@)//Cu = 0.34 V and E_(Cu^(2+))^(@)//Cu^(+) = 0.15 V

Calculate the equilibrium constant for the reaction at 298K. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.76V and E_(Cu^(2+)//Cu)^(@) = +0.34 V