The chemical reaction 2AgCl_((s)) + H_(2(g)) to 2HCl_((aq)) + 2Ag_((s)) taking place in a galvanic cell is represented by the notation.
Depict the galvanic cell in which the reaction Zn(s) + 2Ag^(+) (aq) to Zn^(2+) (aq) + 2A(s) takes place. Further show. (i) Which of the electrode is negatively charged? (ii) The carriers of the current in the cell. (iii) Individual reaction at each electrode.
The standard reduction potentials for the two half-cell reactions are given below : Cd^(2+) (aq) + 2e^(-) to Cd(s) , E^(0) = -0.40 V " "Ag^(+)(aq) + e^(-) to Ag(s) , E^(0) = 0.80 V The standard free energy change for the reaction 2Ag_((aq))^(+) + Cd_((s)) + Cd_((aq))^(2+) is given by
The emf of the involving the reaction 2Ag_((aq))^(+)+H_(2(g)) rarr Ag_((s))+2H_((aq))^(+) is 0.80V . The standard oxidation potential of silver electrode is
Calculate Delta_(r)G for the reaction at 27^(@)C H_(2)(g)+2Ag^(+)(aq)hArr2Ag(s)+2H^(+)(aq) Given : P_(H2)=0.5 bar, [Ag^(+)]=10^(-5)M, [H^(+)]=10^(-3)M,Delta_(r)G^(@)[Ag^(+)(aq)]=77.1kJ//mol
Determine DeltaG^(0) for the button cell used in the watches. The cell reactions is Zn_((s))+Ag _(2)O_((s))H_(2)O _((l))to Zn_((aq))^(2+)+2 Ag _((s))+2OH_((aq))^(-) E_(Ag^(+)//Ag)^(0) =+0.80V,E_(Zn^(2+)//Zn)^(0)=-0.76V.
Determine the values of K_(c) for the following reacton Ni_((s))+2 Ag _((aq))^(+)to Ni_((aq))^(2+)+2Ag _((s)) E^(0) =1.05V.
