The variation of molar conductivity with concentration of an electrolyte $X$ in aqueous solution is shown in the given figure.
The electrolyte $X$ is :

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

Calculate $\Lambda _{HOAc}^{\infty }$ using appropriate molar conductances of the electrolytes listed below at infinite dilution in $H_2O$ at $25\ ^oC$.

Electrolyte	$\Lambda ^{\infty } (S\ cm^2\ mol^{-1})$
$KCl$	$149.9$
$KNO_3$	$145.0$
$HCl$	$426.2$
$NaOAc$	$91.0$
$NaCl$	$126.5$

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 $0.001 \ M$ aqueous solution of $Na_2SO_4$ is found to be $2.6 \times 10^{-3} \ S \ cm^{-1}$ at $25 \ ^oC$. If limiting molar conductance of $Na^+$ is $50 \ S \ cm^2 \ mol^{-1}$,then limiting molar conductance of $SO_4^{2-}$ will be .............. $S \ cm^2 \ mol^{-1}$ (neglect conductivity of water).

The equivalent conductance of a monobasic acid at infinite dilution is $348 \, \Omega^{-1} \, cm^2 \, eq^{-1}$. If the resistivity of the solution containing $15 \, g$ of acid (molar mass $49 \, g \, mol^{-1}$) in $1 \, L$ is $18.5 \, \Omega \, cm$,what is the degree of dissociation of the acid? .............. $\%$