Which of the following solutions has the maximum conductivity?

The specific conductance $(k)$ of $0.02 \ M$ aqueous acetic acid solution at $298 \ K$ is $1.65 \times 10^{-4} \ S \ cm^{-1}$. The degree of dissociation $(\alpha)$ of acetic acid is: [Given: $\lambda_{H^{+}}^{\infty} = 349.1 \ S \ cm^2 \ mol^{-1}$ and $\lambda_{CH_3COO^{-}}^{\infty} = 40.9 \ S \ cm^2 \ mol^{-1}$]

Conductivity of a saturated solution of a sparingly soluble salt $AB$ at $298 \ K$ is $1.85 \times 10^{-5} \ S \ m^{-1}$. Solubility product of the salt $AB$ at $298 \ K$ is. Given $\Lambda_{m}^{\circ}(AB) = 140 \times 10^{-4} \ S \ m^{2} \ mol^{-1}$.

Resistance of a conductivity cell filled with $0.1 \ M$ $KCl$ solution is $100 \ \Omega$ and conductivity of the solution is $1.29 \ S/m$. What will be the value of the cell constant (in $m^{-1}$)?

The equivalent conductance of $1 \, M$ benzoic acid is $12.8 \, \text{mho} \, \text{cm}^2 \, \text{g-eq}^{-1}$. If the molar conductivities of benzoate ion and $H^+$ ion are $42$ and $288.42 \, Omega^{-1} \, \text{cm}^2$ respectively,then the degree of dissociation is .......... $\%$.

What is metallic or electronic conductivity? On what factors does it depend?