Calculate the standard cell potential of the Galvanic cell in which the following reaction takes place: `2Cr(s) + 3Cd^(2+)(aq) rarr 2Cr^(3+)(aq) + 3Cd(s)`. Also calculate the `Delta_rG` and equilibrium constant of the reaction.

Calculate the standard cell potential of the Galvanic cell in which the following reaction takes place: Fe^(2+)(aq) + Ag^+(aq) rarr Fe^(3+)(aq) + Ag(s) . Calculate the Delta_rG and equilibrium constant of the reactions.

Calculate the standard cell potential of the Galvanic cell in which the following reaction takes place: 2Cr(s) + 3Cd^(2+)(aq) rarr 2Cr^(3+)(aq) + 3Cd(s) Also calculate the DeltarG^@ value of the reaction. (Given: E_(Cr^(3+)//Cr) = -0.74V , E_(Cd^(2+)//Cd) = -0.40V and F =96500C//mol )

The cell in which the following reactions occur: 2Fe_(aq)^(3+) + 2I_(aq)^(-) rarr 2Fe_(aq)^(2+) + I_(2(s)) has E_(cell)^@ = 0.236V at 298K.Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

The cell in which the following reaction occur. 2Zn(s)+2Cu^(2+)(aq) rarr 2Zn^(2+)(aq)+2Cu(s)E_(cell)^@=1.10 volt at 298K. Calculate the standard Gibbs energy and the equilibrium constant.

Calculate the emf of the cell in which the following reaction takes place. Ni(s) + 2Ag^+ (0.002 M) rarr Ni^(2+)(0.16M) + 2Ag(s) given that E_(cell)^@ = 1.05V

complete the following reaction Al_2O_3+C rarr

Calculate the emf of the cell at 298K, in which the following reaction takes place: Ni(s) + 2Ag^(+)(aq) (0.001M) rarr Ni^(2+)(aq) (0.160M) + 2Ag(s) (Given that E^@ cell = 1.05V )

Calculate the emf of the cell in which the following reaction takes place. Ni_(s) + 2Ag^+ (0.002 M) rarr Ni^(2+)(0.160M) + 2Ag_(s) Given that E_(cell)^@ = 1.05V

Depict the Galvanic cell in which the reaction takes place as follows: Zn(s) + 2Ag^+(aq) to Zn(2+) + 2Ag(s) The carriers of the current in the cell.

Depict the Galvanic cell in which the reaction takes place as follows: Zn(s) + 2Ag^+(aq) to Zn(2+) + 2Ag(s) Individual reaction at each electrode.