Molar conductivity of $0.02 \ M$ weak acid is $7.92 \ \Omega^{-1} \ cm^2 \ mol^{-1}$ and its molar conductivity at infinite dilution is $232.7 \ \Omega^{-1} \ cm^2 \ mol^{-1}$. Calculate the degree of dissociation of the weak acid.

Assertion: Electrical conductivity of copper increases with increase in temperature.
Reason: The electrical conductivity of metals is due to the motion of electrons.

Two solutions of electrolytes $X$ and $Y$ are taken in two beakers and diluted by adding $500 \ mL$ of water. The molar conductivity $(\Lambda_m)$ of $X$ increases by $1.5$ times,while that of $Y$ increases by $20$ times. What could be the electrolytes $X$ and $Y$?

The resistance of a $0.1 \, N$ solution of a salt is $2.5 \times 10^{3} \, \Omega$. If the cell constant is $1.15 \, cm^{-1}$,what will be the equivalent conductance of the solution in $\Omega^{-1} \, cm^{2} \, eq^{-1}$ (in $.6$)?

If the equivalent conductance of $1 \ M$ benzoic acid is $12.8 \ \Omega^{-1} \ cm^2 \ eq^{-1}$ and the equivalent conductances of benzoate ion and $H^{+}$ ion are $42$ and $288.42 \ \Omega^{-1} \ cm^2 \ eq^{-1}$ respectively,its degree of dissociation is ............. $\%$

The resistance of a $0.5 \, M$ solution of an electrolyte in a cell was found to be $50 \, \Omega$. If the electrodes in the cell are $2.2 \, cm$ apart and have an area of $4.4 \, cm^2$,then the molar conductivity (in $S \, m^2 \, mol^{-1}$) of the solution is: