Define the following terms :
(i) Molar conductivity (),
(ii) Secondary batteries.
(i) Molar conductivity (),
(ii) Secondary batteries.
(i) Molar conductivity () : Molar conductivity is defined as the conductivity due to all the ions produced by dissolving one mole of an electrolyte in solution.
(ii) In secondary batteries, the reactions can be reversed the cell reactions imposing a higher voltage than the E.M.F. of cell (external voltage). These batteries can be recharged by passing
electric current and used again and again.
(ii) In secondary batteries, the reactions can be reversed the cell reactions imposing a higher voltage than the E.M.F. of cell (external voltage). These batteries can be recharged by passing
electric current and used again and again.
Calculate pH of following half-cell. Pt, \(H_2\) / \(H_2\)\(SO_4\) , if its electrode potential is 0.03V.
The conductivity of 0.20 M solution of KCl at 298 K is 0.025 Scm⁻¹. Calculate its molar conductivity.
The conductivity of metals decreases while that of electrolytes increases with increase in temperature. Why?
The potential of a hydrogen electrode at pH = 10 is
a. 0.591 V
b. 0.00 V
c. – 0.591 V
d. -0.059 V
State Kohlrausch law of independent migration of ions. Why does the conductivity of a solution decrease with dilution ?
Calculate emf of the following cell
Cd/\(Cd^{2+}\) (.10 M)//\(H_+\) (.20 M)/\(H_2\) (0.5 atm)/Pt
[Given E° for \(Cd^{2+}\) /Cd = -0.403V]
(i) Following reactions occur at cathode during the electrolysis of aqueous silver chloride solution :
= +0.80 V
= 0.00 V
On the basis of their standard reduction electrode potential (E°) values, which reaction is feasible at the cathode and why ?
(ii) Define limiting molar conductivity. Why conductivity of an electrolyte solution decreases with the decrease in concentration ?
Define the following terms:
(i) Abnormal molar mass
(ii) van’t Hoff factor
Complete the following chemical equations :
(i) MnO₄⁻(aq) + S₂O₃²⁻(aq) + H₂O(l) →
(ii) Cr₂O₇²⁻(aq) + Fe²⁺(aq) + H⁺(aq) →
In the following ions:
Mn³⁺, V³⁺, Cr³⁺, Ti⁴⁺
(Atomic no: Mn = 25, V = 23, Cr = 24, Ti = 22)
(a) Which ion is most stable in an aqueous solution?
(b) Which ion is the strongest oxidizing agent?
(c) Which ion is colourless?
(d) Which ion has the highest number of unpaired electrons?
Calculate the molality of ethanol solution in which the mole fraction of water is 0.88.
What is meant by rate of a reaction ? Differentiate between average rate and instantaneous rate of a reaction.