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`

What is the effect of an increase in concentration of Zinc ions on the electrode potential of Zinc electrode for which E^@ equals -0.76V.

What is the effect of an increase in concentration of zinc ions on the electrode potential of zinc electrode for which E^@ equals to -0.76V.

One half-cell in a voltaic cell is constructed from a silver wire dipped in silver nitrate solution of unknonw concentration. It other half cell consists of a zinc electrode dipping in 1.0M solution of Zn(NO_3)_2 . A voltage of 1.48V is measure for this cell. Use this information to calculate the concentration of silver nitrate solution used (E_(Zn^(2+)//Zn)^0=-0.76V,E_(Ag^+//Ag)^0=+0.80V)

Can we use a Copper Vessel to store 1M AgNO_3 solution? Given that E_(Cu^(2+)//Cu)^@ = 0.34v and E_(Ag^(+)//Ag)^@ = 0.80v

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+)(0.0001 M)|Cu(s)

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

The date below are for the reaction of NO and Cl_2 to form NOCl at 295K. Determine the reaction rate when the concentrations of Cl_2 and NO are 0.2M and 0.4M respectively?

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?