Define the following terms : (i) Fuel cell (ii) Limiting molar conductivity $\Lambda_{m}^{\mathrm{o}}$

Define the following terms : (i) Molar conductivity ($\Lambda_{m}$), (ii) Secondary batteries.

State Kohlrausch law of independent migration of ions. Why does the conductivity of a solution decrease with dilution ?

Calculate the degree of dissociation (α) of acetic acid if its molar conductivity ($\Lambda_{m}$) is 39.05 Scm² mol⁻¹. Given $\Lambda^{\mathrm{o}}$(H⁺) = 349.6 Scm² mol⁻¹ and $\Lambda^{\mathrm{o}}$(CH₃COO⁻) = 40.9 Scm² mol⁻¹..

The conductivity of 0.20 M solution of KCl at 298 K is 0.025 Scm⁻¹. Calculate its molar conductivity.

The conductivity of a 0.01 M solution of acetic acid at 298 K is 1.65 x 10⁻⁴ S cm⁻¹. Calculate molar conductivity ($\Lambda_{m}$) of the solution.

The following curve is obtained when molar conductivity is plotted against the square root of concentration, c½ for two electrolytes A and B :

(i) State the law which helps to determine the limiting molar conductivity of weak electrolyte. (ii) Calculate limiting molar conductivity of CaSO₄ (limiting molar conductivity of calcium and sulphate ions are 119.0 and 160.0 Scm² mol⁻¹ respectively)

The electrical resistance of a column of 0.05 M KOH solution of diameter 1 cm and length 45.5 cm is 4.55 × 10³ ohm. Calculate its molar conductivity.

Calculate the molar conductivity and degree of dissociation. Conductivity of 2.5 × 10⁻⁴M methanoic acid is 5.25 × 10⁻⁵ Scm⁻¹. Given : $\Lambda^{0}(\mathrm{H}^{+})=349.5\,\mathrm{S}\,\mathrm{cm}^{2}\,\mathrm{moI}^{-1}\,\mathrm{and}\,\Lambda^{0}(\mathrm{HCOO}^{-})$ = 50.5Scm² mol⁻¹

When a certain conductance cell was filled with 0.1 M KCl, it has a resistance of 85 ohm at 25°C. When the same cell was filled with an aqueous solution of 0.052 M unknown electrolyte, the resistance was 96 ohms. Calculate the molar conductance of the electrolyte at this concentration. [Specific conductance of 0.1 M KCl = 1.29 × 10⁻² ohm⁻¹ cm⁻¹]

(i) Following reactions occur at cathode during the electrolysis of aqueous silver chloride solution : $\mathbf{Ag}^{+}(\mathbf{aq})+\mathbf{e}^{-}\rightarrow\mathbf{Ag}(\mathbf{s})\qquad\qquad\mathbf{E}^{\circ}$ = +0.80 V $\mathrm{H}^{+}(\mathrm{aq})+\mathrm{e}^{-}\rightarrow\frac{1}{2}\mathrm{H}_{2}(\mathrm{g})~~~~~~~~~\mathrm{E}^{\circ}$ = 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 ?

In a galvanic cell, the following cell reactions occurs: $\mathbf{Zn}(s)+2\mathbf{A}\mathbf{g}^{+}(\mathbf{a}\mathbf{q})\rightarrow\mathbf{Zn}^{2+}(\mathbf{a}\mathbf{q})+2\mathbf{A}\mathbf{g}(s)$ E°cell = +1.56 V (i) Is the direction of flow of electrons from zinc to silver or silver to zinc? (ii) How will concentration of Zn²⁺ ions and Ag⁺ ions be affected when the cell functions?

Following reactions can occur at cathode during the electrolysis of aqueous silver nitrate solution using Pt electrodes: