Write balanced equations for the half reactions and calculate the reducation potentials at `25^@C` for the following half cells : `Cl^- (1.2 M)|Cl_2 (g), 3.6 atm l Pt, E^@ = 1.36 V`

Write balanced equations for the half reactions and calculate the reducation potentials at 25^@C for the following half cells : Fe^(2+)(2M)|Fe_((s)),E^@=-0.44V .

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

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 the potential of the following cell at 25^@C . Sn_((s))|Sn^(2+) (0.025M)||Ag^+ (0.015M)|Ag(s) E_(sn)^0 = -0.136V, E_(Ag)^@ = 0.799V .

Consider a galvanic cell that uses the half reactions: 2H_((aq))^+ +2e^- rarr H_(2(g)) Mg_((aq)) +2e^-rarrMg_((a)) Write balanced equation for the cell reaction. Calculate E_(Cell)^@ and DeltaG^@ if concentrations are 1M each and P_(H2)=10 atm. E_(Mg)^@=-2.37V .

Balance the following chemical equations: P_(4(s))+Cl_(2(g))rarr PCl_(3(l))

The standard reduction potentials at 25^(@)C for the following half reactions are given against each: Zn^(2+) (a.q) + 2e^(-) rarr Zn (s) : " " - 0.762 Cr^(3+) (a.q) 3e^(-) rarr Cr (s) , " " - 0.740 2H^(+) + 2e^(-) rarr H_(2) (g), " " 0.00 Fe^(3+) + e^(-) rarr Fe^(2+) , " " 0.77 Which is the strongest reducing agent?

The balancing lengths for the cells of emfs E_1 and E_2 are l_1 and l_2 respectively . If they are connected separately then