E.m.f of the cell
`2Ag^(+) + Cu rightarrow Cu^(+2) = 2Ag`
[Given : E^(@) `= -0.8V , E^(@)_(Cu^(+2) Cu = 0.3V]`

E.M.F of the cell reaction , 2Ag^(+) + Cu to 2Ag + Cu^(2+) is 0.46 V . If E_(Cu^(2+) // Cu)^(0) is | 0.34 V , E_(Ag^(+)//Ag)^(0) is

The cell reaction of a cell is Mg+Cu^(2+) to Mg^(2+)+Cu (Given E_(Mg^(2+)//Mg) = -2.37 V , E_(Cu^(2+)//Cu) = 0.337 V ) The e.m.f of the cell will be _________.

The equilibrium constant for the cell Cu(s)+2Ag^+(aq)rarrCu^(2+)(aq)+2Ag(s) ,at 298K is [Given, E_((Ag)^+/(Ag))^o=0.8V and E_((Cu)^(2+)/(Cu))^o=0.34V ]

The equilibrium constant for the cell Cu(s)+2Ag^+(aq)rarrCu^(2+)(aq)+2Ag(s) ,at 298K is [Given, E_((Ag)^+/(Ag))^o=0.8V and E_((Cu)^(2+)/(Cu))^o=0.34V ]

The e.m.f. of the cell at 25^(@)C Cu"|"Cu^(2+)(0.01M)"||"Ag^(+)(0.1M)"|"Ag is [E^(@)(Cu^(2+)"|"Cu)=0.34V, E^(@)(Ag^(+)"|"Ag)=0.80V]

Is it safe to stir 1M AgNO_(3 ) solution with copper spoon? Given: E^(@)Ag^(+)//ag=0.80V,E^(@)Cu^(2+)//Cu^(2+)//Cu=0.34V

Determine DeltaG^(@) and the value of the equilibrium constant for the following reaction occurring in an electrochemical cell at 25^(@)C . Cu(s)+2Ag^(+)(aq)rarr Cu^(2+)(aq)+2Ag(s) Given that, E_(Cu^(2+)|Cu)^(@)=0.34V and E_(Ag^(+)|Ag)^(@)=0.80V