The specific conductance of a $0.01 \, M \, KCl$ solution at $25 \, ^{\circ}C$ is $0.0014 \, \Omega^{-1} \, cm^{-1}$. Its equivalent conductance is ..... (in $\Omega^{-1} \, cm^{2} \, eq^{-1}$).

The limiting molar conductivities of the given electrolytes at $298 \ K$ follow the order: $\lambda^{\circ}_{(K^{+})} = 73.5, \lambda^{\circ}_{(Cl^{-})} = 76.3, \lambda^{\circ}_{(Ca^{2+})} = 119.0, \lambda^{\circ}_{(SO_{4}^{2-})} = 160.0 \ S \ cm^{2} \ mol^{-1}$.

$0.0129 \ S \ cm^{-1}$ is equivalent to how many $S \ m^{-1}$ (in $S \ m^{-1}$)?

Which of the following has maximum conductivity in solution?

$A$ $KCl$ solution of conductivity $0.14 \, S m^{-1}$ shows a resistance of $4.19 \, \Omega$ in a conductivity cell. If the same cell is filled with an $HCl$ solution,the resistance drops to $1.03 \, \Omega$. The conductivity of the $HCl$ solution is $....... \, \times 10^{-2} \, S m^{-1}$. (Round off to the Nearest Integer).

Explain the conduction of electricity in metals and non-metals.