What will be the half cell rection for bromine electrode represented by `Pt(s)//Br_2(aq).Br^(-)(aq)`?

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.

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)

Write the Nernst equation and emf of the following cells at 298K. pt(s)|Br_2(l)|Br^(-)(0.010M)||H^+(0.030M)|H_2(g)(1bar)pt(s) .

Write the Nernst equation and emf of the following cells at 298K. pt(s)|Br_2(l)|Br^(-)(0.010M)||H^+(0.030M)|H_2(g)(1bar)pt(s) .

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 Delta_rG and equilibrium constant of the reaction.

Following are the data of standard reduction half cell potentials of certain electrochemical cells. E_(Ag^(+)//Ag)^@ = 0.80V & E_(Cu^(2+)//Cu)^@ = 0.34V E_(Sn^(2+)//Sn)^@ =-0.14V & E_(Na^(2+)//Na)^@ = -2.71V Represent the electrochemical cell constructed from these pair of half cells.

Calculate the equilibrium constant of the following reaction aty 298K. Cu(s)+2Ag^+(aq) rarr Cu^(2+)(aq)2Ag(s)~ Given E_(cell)^Theta=0.46V

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 equilibrium constant for the following reaction. Fe(s)+2Ag^+(aq) rarr 2Ag(s)+Fe^(2+)(aq) E_(Fe^(2+)//Fe)^@=-0.44V,E_(Ag^+//Ag)^=+0.80V .