COnsider an electrochemical cell pt, `H_2` | `H^+`|| `Ag^+`| `Ag` Given , `E^o`(`Ag^+`|Ag)= +0.80V the value of delta `G^o` for the cell represented above is -x Kj then the value of x in nearest integer is ?

Standard electrode potential of cell H_2 ||H^+ || Ag^+ | Ag is ,.

For the cell Pt | H_(2) | HCl|| Ag^(+) | Ag , E_(cell) can be increased by:

Calculate emf of given cell at 25^(@)C : [Given: E_(Ag^(+)//Ag)^(@)) = 0.80V]

The following chemical reaction occurring in an electrochemical cell : Mg(s)+2Ag^(+)(0.0001 M) to Mg^(2+)(0.10 M)+2Ag(s) Given E_(Mg^(2+)//Mg)^(@)=-2.36" V", E_(Ag^(+)//Ag)^(@)=+0.81" V" For the cell, calculate/write : (i) E^(@) value for the electrode 2Ag^(+)//2Ag (ii) Standard cell potential (E^(@)) (iii) Cell potential (E) (iv) Give the symbolic representation of the above cell (v) Will the above cell reaction be spontaneous ?

Calculate the following cell reaction cell at 298 K. 2Ag^(+)+Cd to 2Ag+Cd^(2+) E^(@) for Ag^(+)//Ag and Cd^(2+)//Cd are 0.80 V and -0.40 V respectively. E^(@) for Ag^(+)//Ag and Cd^(2+)//Cd are 0.80 V and -0.40 V respectively. (i) Write the cell representation. (ii) What will be the emf of the cell if the concentration of Cd^(2+) is 0.1 M ? (iii) Will the cell work spontaneously for the condition given above ?