The conductivity of metals decreases while that of electrolytes increases with increase in temperature. Why?

The conductivity of an aqueous solution of NaCl in a cell is 92 \(Ω^{−1}\) \(cm^{-1}\) the resistance offered by this cell is 247.8 Ω . Calculate the cell constant.

How many electrons flow when a current of 5 amps is passed through a solution for 193 sec ? Given F = 96500 C. \(N_0\) = 6.002 × \(10^{23}\) \(mol^{-1}\).

There are two possible reactions for cathode in the electrolysis of aqueous \(ZnCl_2\) :\(Zn^{2+}\) (aq) + 2\(e^-\) → Zn(s) \(E^0\) = -0.76 V 2\(H_2\)O (l) + 2\(e^-\) → H2 (g) + 2\(OH^-\) (aq) \(E^0\) = - 0.83 V Which one will take place? Why?

Calculate pH of following half-cell. Pt, \(H_2\) / \(H_2\)\(SO_4\) , if its electrode potential is 0.03V.

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)

(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?