For the cell, `Zn|ZnO_(4)||AgNO_(3)|Ag`, the cell reaction is : `Zn+2Ag^(+)rarr Zn^(2+)+2Ag.` If `E_("cell")^(@)=+0.36V`, then calculate `Delta^(@)` for the cell reaction of that cell.

The cell reaction Zn+2Ag^+ rarrZn^(2+)+2Ag is best represented by

The cell reaction, Zn + 2Ag_(aq)^+ rarr Zn^(+2) Ag can be represented by

The cell reaction Zn(s)+2Ag^(+)(aq)rarrZn^(2+)(aq)+2Ag(s) is best represented by

The emf of the cell, Zn|Zn^(2+)|Ag^(+)|Ag is independent of

The emf of the cell, Zn|Zn^(2+)|Ag^(+)|Ag is independent of

Represent the cell with cell reaction- Zn(s)+2Ag^+(aq) rarr Zn^(2+) (aq)+2Ag(s) Calculate the emf of the cell at 298K if the molar concentraction of Ag^+ and Zn^(2+) ions in the half cwells are 0.10 mol dm^(-3) and 0.01 mol dm^(-3) respectively. Given that E^@ Ag^+//Ag= 0.80V and E^@Zn^(2+)//Zn=-0.76V,

Calculate the emf of the cell having the cell reaction 2Ag^(+)+ZnhArr 2Ag+Zn^(2+) and E_("cell")^(@)=1.56V" at "25^(@)C when concentration of Zn^(2+)=0.1M and Ag^(+)=10M in the solution.

Calculate the emf of the cell having the cell reaction 2Ag^(+)+ZnhArr 2Ag+Zn^(2+) and E_("cell")^(@)=1.56V" at "25^(@)C when concentration of Zn^(2+)=0.1M and Ag^(+)=10M in the solution.