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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Similar Questions
$A$ gas deviates most from ideal behavior when it is subjected to
If $Z$ is a compressibility factor,the van der Waals equation at low pressure can be written as:
$A$ gas is said to behave like an ideal gas when the relation $PV/T = \text{constant}$. When do you expect a real gas to behave like an ideal gas?
MediumIIT 1999
View SolutionThe figure represents $PV$ vs $P$ relation for $CO$,$CH_4$,$H_2$ and $He$ gases under identical conditions. Which curve,shown in the figure,represents $He$ gas?
Consider the following table:
Gas $a / (kPa \cdot dm^6 \cdot mol^{-2})$ $b / (dm^3 \cdot mol^{-1})$ $A$ $642.32$ $0.05196$ $B$ $155.21$ $0.04136$ $C$ $431.91$ $0.05196$ $D$ $155.21$ $0.4382$
$a$ and $b$ are van der Waals constants. The correct statement about the gases is:
| Gas | $a / (kPa \cdot dm^6 \cdot mol^{-2})$ | $b / (dm^3 \cdot mol^{-1})$ |
|---|---|---|
| $A$ | $642.32$ | $0.05196$ |
| $B$ | $155.21$ | $0.04136$ |
| $C$ | $431.91$ | $0.05196$ |
| $D$ | $155.21$ | $0.4382$ |
$a$ and $b$ are van der Waals constants. The correct statement about the gases is:
DifficultJEE MAIN 2019
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