Calculate, emf of the cell at `25^@C Zn(s)|Zn^(2o+)(0.2M)|| H^(o+)(1.6M)|H_2(g, 1.8 atm)|Pt`

Calculate emf of the cell Zn_((s))|Zn^(2o+) (0.2M)|Ho+ (1.6M)H_2(g.1.8atm)|Pt^(a)t 25^@C .

Calculate the potential of the following cell at 25^@C . Zn|Zn^(2+)(0.6M)||H^+(1.2M)|H_2(g, 1 atm)|Pt E_(Zn)^@=-0.763V .

Calculate emf of the following cell at 25^@C . Zn((s))|Zn^(2o+)(0.08M)||Cr^(3o+)(0.1M)|Cr E_(Zn)^0=-0.76V, E_(Cr)^0=-0.74V)

Calculate the voltage of the cell, Sn (s)|Sn^(2o+) (0.02M) || Ag^(o+) (0.01M)|Ag (s) at 25^@C . E^@= -0.136 V, E_(Ag)^@= 0.800 V .

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)) (Given E_(Fe^(2+)//Fe)^0=-0.440V)

Write the cell reaction and calculate the standard potential of the cell. Ni_((s))|Ni^(2+) (M)||CI (1M)|CI_2 (g.latm)|Pt E_(Cl2)^@ = 1.36 V and E_^@ = -0.25 V

Write the Nernst equation and emf of the following cells at 298 K. Pt_((s))|Br_(2(1))|Br^- (0.010M)||H^+(0.030 M)|H_(2(g)) (1 bar)|Pt_((s)) (Given E_(Br^-)^@ = + 1.08 V)

Write the Nernst equation and emf of the following cells at 298 K. Sn_((s))|Sn_(aq)^2+(0.050M)|H_(aq)^+(0.020 M)|H(2(g))(1 bar)Pt_((s)) (Given E_(Sn^(2+)//Sn)^0 =- 0.136 V)