What will happen to the value of emf of the cell `Zn|Zn^(2+)(0.1M)||Cu^(2+)(0.1 M)|Cu`, if the concentration of the electrolyte in the anode compartment is increased?

Write the Nernst equation of the following cell Mg(s)|Mg^(2+)(0.001M)||Cu^(2+)(0.0001M)|Cu(s)

Write the Nernst equation and emf of the following cells at 298K. Mg(s)|Mg^(2+)(0.001 M)||Cu^(2+)(0.001 M)|Cu(s)

Write the Nernst equation and emf of the following cells at 298K. Mg(s)|Mg^(2+)(0.001 M)||Cu^(2+)(0.0001 M)|Cu(s)

The measured emf of the cell- Pt(s)H_2(G,1bar)|H^+(aq,1M)|| Cu^(2+)(aq,1M)|Cu(s)is 0.34V . What is the standard electrode potential of the half cell corresponding to the reaction?

A cell is represented in the following way. Cu(s)|Cu^(2+)(aq)||Ag^+(aq)|Ag(s) name the electrolytes required for the above cell.

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,

A copper silver cell is set up. The copper ion concentration is 0.10M . The concentration of silver ion is not known. The cell potential when measured was 0.422V. Determine the concentration of silver ions in the cell. (Given) E_(Ag^(2+)//Ag)^@=+0.80V,E_(Cu^(2+)//Cu)^@=+0.34V

For what value of m will the equation x^2 -(3m - 1) x + 2m^2 + 2m - 11 =0 have equal roots? Find the roots.

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

Write the Nernst equation and emf of the following cells at 298K. Fe(s)|Fe^(2+)(0.001M)||H^+(1M)|H_2(g)(1 bar)|pt(s)