The partial molar volumes of benzene $(1)$ and carbon tetrachloride $(2)$

equimolar mixtures are, at a given temperature, $\frac{?}{\text{b}\text{a}\text{r}}(V{)}_1=0\mathrm{.}116d{m}^3*mo{l}^{-1}$ and

$\frac{?}{\text{b}\text{a}\text{r}}(V{)}_2=0\mathrm{.}102d{m}^3*mo{l}^{-1}.$

a$.$ Calculate the volume of a mixture consisting of five moles of each

compound at that temperature.

b$.$ Calculate the volumetric mass of that mixture in units of $kg$ per

$m^3.$ The benzene molar mass is $78\mathrm{.}11g*mo{l}^{-1}$ and for carbon

tetrachloride is $78\mathrm{.}11g*mo{l}^{-1}.$

c$.$ Calculate the excess volume during the mixing of $5$mol of benzene

and $5$mol of carbon tetrachloride. Interpret in terms of

interactions in solution. The molar volumes of the pure components

are: $,V_1=0\mathrm{.}087d{m}^3*mo{l}^{-1}$ e $V_2=0\mathrm{.}098d{m}^3*mo{l}^{-1}.$