Calculate the electrode potential at a copper electrode dipped in 0.1 M solution of copper sulphate at `25^@C`. Given, the standard emf of `Cu^(2+)` system is +0.34V at 298K.

Calculate the electrode potential of a copper electrode dipped in 0.1M solution of copper sulphate at 25^@C . (Given E^@ for Cu is +0.34V at 298K)

The hydrogen electrode is dipped in a solution of pH= 3 at 25^@C . The potential of the cell is given by.

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)

When a metal rod C in dipped in an aquos soluion of a metal D (having conentration 1M for D^(2+) ion) at 25^@C the standard electrode potential are C^(2+)//C=-0.76 volts. D^(2+)D=+0.34 volts .

The standard electrode potential for Daniel cell is 1.1V. Calculate the standard Gibb's energy for the reaction. Zn_(s)+ Cu_(aq)^(2+) rarr Zn_(aq)^(2+)+Cu_(s) .

The electrode potentials for the two half cell reaction is given below. Determine emf Mg^(2+)+2e^- rarr Mg(s), E=-2.37V Cu^(2+)+2e^- rarr Cu(s), E=+0.34V.

Calculate the entropy change in surrounding when 1 mol of H_2O(l) is formed under standard condition at 298K. Given Delta_fH^@ =-286KJ mol^(-1)

Which of the following pairs will have greater conduction ? 0.1M NaCl solution at 25^@C and 0.1M NaCl solution at 50^@C .