[" The emf of the cell,"],[" Ag "|Ag^(+)(0.1M)|Ag^(+)(1M)|Ag" at "298K" is "]

The e.m.f. of the cell : Cu(s)"|"Cu^(2+)(1M)"||"Ag^(+)(1M)"|"Ag is 0.46 V. The standard reduction reduction potential of Ag^(+)//Ag is 0.80 V. The standard reduction potential of Cu^(2+)//Cu is

Calculate the emf of the cell. Zn|Zn^(2+)(0.001M)||Ag^(+)(0.1M)|Ag The standard potential of Ag//Ag^(+) half - cell is +0.80 V and Zn//Zn^(2+) is -0.76V.

Calculate the emf of the cell. Zn|Zn^(2+)(0.001M)||Ag^(+)(0.1M)|Ag The standard potential of Ag//Ag^(+) half - cell is +0.80 V and Zn//Zn^(2+) is -0.76V.

Find the solubility product of a saturated solution of Ag_2CrO_4 in water at 298 K if the e.m.f of the cell : [Ag|Ag^+ (sat. Ag_2CrO_4)|Ag^+ (0.1M)|Ag is 0.164 Vat 298 K .

Given that (at T = 298 K) Cu(s) | Cu^(2+)(1.0M) || Ag^(+)(1.0M)| Ag(s) underset(E_(cell)^(@) = 0.46V Zn(s) | Zn^(2+) (1.0M) || Cu^(2+) (1.0M) | Cu(s) underset(E_(cell)^(@) = 1.10V Then E_(cell) for, Zn | Zn^(2+)(0.1M) || Ag^(+)(0.1M) | Ag at 298 K will be:

Given that (at T = 298 K) Cu(s) | Cu^(2+)(1.0M) || Ag^(+)(1.0M)| Ag(s) underset(E_(cell)^(@) = 0.46V Zn(s) | Zn^(2+) (1.0M) || Cu^(2+) (1.0M) | Cu(s) underset(E_(cell)^(@) = 1.10V Then E_(cell) for, Zn | Zn^(2+)(0.1M) || Ag^(+)(1.0 M) | Ag at 298 K will be:

The emf of the cell, Ni|Ni^(2+)(1.0M)||Ag^(+)(1.0M)|Ag [E^(@) for Ni^(2+)//Ni =- 0.25 volt, E^(@) for Ag^(+)//Ag = 0.80 volt] is given by : [E^(@) for Ag^(+)//Ag = 0.80 volt]