A mole of $C C l_{4}$ vapours at $77^{\circ} C$ occupies a volume of 36.0 L.If vanderwaals constants are $a = 20.39 L^{2} a t m m o l^{- 2}$ and $b = 0.1383 L m o l^{- 1}$ calculate the compressibility factor Z under (a) low pressure region and (b) high pressure region.
The values of compressibility factor Za and Zb respectively are:

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The denisity of water vapour at 240 atm and 527∘C is 90gm/dm3. Determine the molar volume(vm) of water and the compression factor.[Use :R=0.08 atmL/molK]

The correct option is D None of theseMolar volume Vn=RTPVn=0.08×800240=0.267L/molThe compressibility factor Z=PVRT=240×0.2670.08×800=1

The denisity of water vapour at 240 atm and $527^{\circ} C$ is $90 g m / d m^{3}$ . Determine the molar volume $(v_{m})$ of water and the compression factor.
[Use :R=0.08 atmL/molK]

The correct option is D None of these
Molar volume $\frac{V}{n} = \frac{R T}{P}$

$\frac{V}{n} = \frac{0.08 \times 800}{240} = 0.267 L / m o l$

The compressibility factor $Z = \frac{P V}{R T} = \frac{240 \times 0.267}{0.08 \times 800} = 1$