If $0.01 \, M$ solution of an electrolyte has a resistance of $40 \, \Omega$ in a cell having a cell constant of $0.4 \, cm^{-1}$,then its molar conductance in $ohm^{-1} \, cm^2 \, mol^{-1}$ will be :-

Resistance of a decimolar solution between two electrodes $0.02 \ m$ apart and $0.0004 \ m^2$ in area was found to be $50 \ \Omega.$ Specific conductance $(\kappa)$ is .......... $S \ m^{-1}$

Molar conductivity of $0.01 \ M \ CH_3COOH$ is $19.5 \ \Omega^{-1} \ cm^2 \ mol^{-1}$. Calculate its degree of dissociation if molar conductivity at zero concentration is $390 \ \Omega^{-1} \ cm^2 \ mol^{-1}$.

The molar conductance of an infinitely dilute solution of ammonium chloride was found to be $185 \ S \ cm^2 \ mol^{-1}$ and the ionic conductance of hydroxyl and chloride ions are $170$ and $70 \ S \ cm^2 \ mol^{-1}$,respectively. If molar conductance of $0.02 \ M$ solution of ammonium hydroxide is $85.5 \ S \ cm^2 \ mol^{-1}$,its degree of dissociation is given by $x \times 10^{-1}$. The value of $x$ is $...........$ $(Nearest \ integer)$

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 $m^{-1}$)?

Which of the following expressions represents the molar conductivity of an $AB_3$ type electrolyte?