Calculate the EMF of the electrode concentration cell Hg-Zn `(c_(1)M)|(Zn^(2+)(c M)|` Hg-Zn `(c_(2)M)` at `25^(@)C`, if the concentration of the zinc amalgam are 2 g per 100 g of mercury and 1g per 100 g of mercury in anode and cathode half-cell respectively.

Calculate the e.m.f of the following concentration cell at 298K, Zn(s)| Zn^(2+)(0.1) || Zn^(2+) (1.0)|Zn(s)

In a concentration cell, Zn|Zn^(2+) (0.1M) || Zn^(2+) (0.15M) | Zn , as the cell discharges:

Galvanic cells generate electrical energy at the expense of a spontaneous redox reaction. In an electrode concentration cell two like electrodes having different concentrations, either because they are gas electrodes operating at different pressures or because they are amalgams (solutions in mercury) with different concentrations are dipped into the same solution. Eg. An example is a cell composed of two chlorine electrodes with different pressure of Cl_(2) : Pt_(L)|Cl_(2)(P_(L))|HCl(aq)|Cl_(2)(P_(R))|Pt_(R) Where P_(L) and P_(R) are the Cl_(2) pressure at the left and right electrodes. Calculate the EMF of the electrode concentration cell represented by : Hg-Zn(c_(1))|Zn^(+2)(aq)|Hg-Zn(c_(2)) At 25^(@)C.c_(1)=2g of Zn per 100g of Hg and c_(2)=1g of Zn per 50g of Hg

Galvanic cells generate electrical energy at the expense of a spontaneous redox reaction. In an electrode concentration cell two like electrodes having different concentrations, either because they are gas electrodes operating at different pressures or because they are amalgams (solutions in mercury) with different concentrations are dipped into the same solution. Eg. An example is a cell composed of two chlorine electrodes with different pressure of Cl_(2) : Pt_(L)|Cl_(2)(P_(L))|HCl(aq)|Cl_(2)(P_(R))|Pt_(R) Where P_(L) and P_(R) are the Cl_(2) pressure at the left and right electrodes. Calculate the EMF of the electrode concentration cell represented by : Hg-Zn(c_(1))|Zn^(+2)(aq)|Hg-Zn(c_(2)) At 25^(@)C.c_(1)=2g of Zn per 100g of Hg and c_(2)=1g of Zn per 50g of Hg

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.