Calculate the Δr G° and the equilibrium constant for the reaction
2Cr(s) + 3Cd2+ (aq) 2Cr3+ (aq) + 3Cd(s)
(Given E°Cr3+/Cr = 0.74 V, E°Cd2+/ Cd = – 0.40 V)
∴
Calculate the cell e.m.f. and ΔG for the cell reaction at 298 K for the cell
Zn(s) | Zn2+ (0.0004 M) || Cd2+(0.2 M) | Cd(s)
(Given E°Zn2+/Zn = 0.763 V, E°cd 2+ / cd = 0.403 Vat 298 K, F = 96500 C mol–1)
(i) According to nernst equation:
(ii)
State whether the following statements are true (T) or false (F):
A.
According Kohlrausch law the value of Λ°m of an electrolyte AB2 which dissociates as A2++ 2B– is given by λ°A+ + λB–
B.
The amount of electricity required to deposit 1 mol of aluminium from a solution of AlCl3 will be 3F.C.
The molar conductivity of an electrolyte increases as concentration decreases.D.
During the discharging of lead storage battery the density of H2SO4 decreases.E.
Daniell cell converts the heat released during the combustion of H2 to an electrical energy.State whether the following statements are true (T) or false (F):
A.
A cell is feasible if its Ecell is negative.B.
The cell constant is independent of the concentration of the electrolyte in the conductivity cell.C.
In recharging of lead storage battery sulphuric acid is produced.D.
The half-cell H+ (0.5)/1/2 H2 (g) (1 atm)/Pt has zero electrode potential.E.
The dependence of electrode potential for the electrode Mn+/ M with concentration under STP condition is given by expression.