Calculate emf of given cell at `25^(@)C`:

[Given: `E_(Ag^(+)//Ag)^(@)) = 0.80V]`

The standard potential of the following cell is 0.23 V at 15^@C and 0.21V at 35^@C (Pt) H_2(g) |HCl(aq)|AgCl(s)|Ag(s) Calculate the solubility of AgCl in water at 25^@C Given: E_(Ag^+,Ag)^@=0.80V at 25^@C

A cell is set up between copper and silver as follows : Cu(s)|Cu^(2+)(aq)||Ag^(+)(aq)|Ag(s) If two half cells work under standard conditions, calculate the emf of the cell. Given E_(Cu^(2+)|Cu)^(@)=0.34V,E_(Ag^(+)//Ag)^(@)=0.80V

Calculate the emf of the cell at 298K E_(NI^(2+)//NI)^0 is -0.25V and E_(Ag^+//Ag)^0 is +0.80V .

Standard electrode potentials are given as, E_(Cu^(2+)//Cd)^(@)=0.34" V " " and " E_(Ag^(+)//Ag)^(@)=0.80" V " Calculate the cell potential, E for cell containing 0.100 M Ag^(+) and 4.00 M Cu^(2+) at 25^(@)C .

Calculate standard free energy change for the reaction 2Ag+2H^(+)rarrH_(2)+2Ag^(+) Given : E_(Ag^(+)//Ag)^(@)=+0.80V

Calculate standard free energy change for the reaction 2Ag+2H^(+)rarrH_(2)+2Ag^(+) Given : E_(Ag^(+)//Ag)^(@)=+0.80V