I_(2)(s) | I^(-) (0.1M) half cell is connected to a H^(+)(aq) | H_2("1 bar ") | Pt half cell and e.m.f is found to be 0.7714 V . If E_(I_2|I^(-))^(@) = 0.535 V , find the pH of H^(+) | H_2 half - cell .
Write the Nernst equation and emf of the following cells at 298 K: (i) Mg(s)|Mg^(2+) (0.001M)|Cu^(2+)(0.0001 M)|Cu(s) (ii) Fe(s)|Fe^(2+)(0.001M)|H^(+) (1M)|H_(2)(g) (1bar) | Pt(s) (iii) Sn(s)|Sn^(2+) (0.050 M)|H^(+)(0.020 M)|H_(2)(g) (1 "bar" )|Pt(s) (iv) Pt(s) |Br_(2)(l) |Br^(-)(0.010 M) |H^(+)(0.030 M)|H_(2)(g) (1 "bar"))|Pt(s) .
Calculate the emf of the cell at 298 K Sn_((s))|Sn^(2+)(0.05M)||H_((aq))^(+)(0.02M) |H_(2) 1 atm. Pt Given that E_(sn^(2+)//Sn)^(0)=-0.144V
Calculate the emf of the cell Cu(s) | Cu^(2+) (aq) || Ag^(+)(aq) | Ag(s) Given, E_((Cu^(2+))//(Cu))=+ 0.34 V, E_((Ag^(+))//( Ag)) = 0.80 V
For the cell , Hg,Hg_2 Cl_2//Cl (0.1M)//Cl^(-)(0.01M)//Cl_2, Pt E_("cell")^@ is 1.10V , Hence , E_("cell") is
Calculate the emf of the cell at 25^(@)C Cr|Cr^(3+)(0.1M)||Fe ^(2+)(0.01M) |Fe, given that E_(Cr^(3+)//Cr )^(0)=-0.74V and E_(Fe ^(2+)//Fe )^(0)=-0.44V
Calculate the EMF of cell Ni//Ni^(2+) (0.01M)"//"Cl^(-)0.1M//Cl_(2) , Pt E^(@)Ni^(2+)//Ni= -0.250V : E^(@)Cl_(2)//Cl^(-)= +1.360V
The emf of the following cell Mg | Mg^(+2) (0.01 M) || Sn^(+2) (0.1 M) | Sn at 298 K in 'V' is (Given , E_(Mg^(+2)|Mg)^(@) = -2.34 V, E_(Sn^(+2)|Sn)^(@) = - 0.14 V )
Represent the cell in which the following reaction takes place Mg(s)+2Ag^(+)(0.0001M) to Mg^(2+) (0.130M)+2Ag(s) Calculates its E_(cell) if E_("cell")^(Θ)=3.17V
Represent the cell in which the following reaction takes place . Mg(s) + 2Ag^(+)(0.001M) to Mg^(2+) (0.130M) + 2Ag(s) . Calculate its E_(("cell")) if E_(("cell"))^(-) = 3.17 V .