Define the compressibility factor $(Z)$ in terms of the molar volume of a gas.
- A$Z = \frac{V_{m, real}}{V_{m, ideal}}$
- B$Z = \frac{V_{m, ideal}}{V_{m, real}}$
- C$Z = V_{m, real} \times V_{m, ideal}$
- D$Z = V_{m, real} + V_{m, ideal}$
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Which statement is correct regarding a real gas?
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View SolutionWhich gas among the following is the easiest to liquify?
At low pressure,Vander Waal's equation is reduced to $\left[ P + \frac{a}{V^2} \right]V = RT$. The compressibility factor $(Z)$ can be given as
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View SolutionThe following data is obtained for one mole of a gas. The gas deviates from ideal behavior in the pressure (in bar) range:
$P \text{ (bar)}$ $\frac{PV}{RT}$ $1$ $1$ $2$ $1$ $3$ $1$ $3.1$ $1.2$ $3.5$ $1.4$ $4.0$ $1.5$
| $P \text{ (bar)}$ | $\frac{PV}{RT}$ |
|---|---|
| $1$ | $1$ |
| $2$ | $1$ |
| $3$ | $1$ |
| $3.1$ | $1.2$ |
| $3.5$ | $1.4$ |
| $4.0$ | $1.5$ |
At high pressure,the form of Van der Waals equation becomes
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