Depict the galvnic cell in which the reaction Zn(s) + 2Ag^+(aq) rarr Zn^(2+)(aq) + 2Ag(s) takes place. Further show: Which of the electrode is negatively charged?

Depict the galvnic cell in which the reaction Zn(s) + 2Ag^+(aq) rarr Zn^(2+)(aq) + 2Ag(s) takes place. Further show: Individual reaction at each electrode.

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.

Depict the Galvanic cell in which the reaction takes place as follows: Zn(s) + 2Ag^+(aq) goes to Zn(2+) + 2Ag(s) Which of the electrode is negatively charged?

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 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 )

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.

Represent the cell in which the following rection takes place. Mg(s) + 2Ag^+(0.01M)rarr Mg^(2+)(0.140M)+2Ag(s) Write the Nemst equation and calculate the emf if the cell at 298K . Given E_(cell)^Theta=3.17V