Compressibility factor,$Z$,of a gas is given as $Z = \frac{pV}{nRT}$.
$(i)$ What is the value of $Z$ for an ideal gas?
$(ii)$ For a real gas,what will be the effect on the value of $Z$ above Boyle's temperature?
$(i)$ What is the value of $Z$ for an ideal gas?
$(ii)$ For a real gas,what will be the effect on the value of $Z$ above Boyle's temperature?
(N/A) $(i)$ For an ideal gas,the compressibility factor is $Z = 1$.
$(ii)$ Above Boyle's temperature,real gases show positive deviation from ideal behavior.
Therefore,for real gases above Boyle's temperature,$Z > 1$.
$(ii)$ Above Boyle's temperature,real gases show positive deviation from ideal behavior.
Therefore,for real gases above Boyle's temperature,$Z > 1$.
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Similar Questions
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
View SolutionThe graph between $P$ and $V$ below the critical temperature is:
MediumAIIMS 2019
View SolutionFor $1$ mol of a real gas kept at constant temperature $T$,the graph of $PV$ vs $P$ intersects the $PV$ axis at $20$. Hence,the temperature $T$ is ($R$ = universal gas constant).
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View Solution$A$ gas deviates most from ideal behavior when it is subjected to
When is deviation more in the behaviour of a gas from the ideal gas equation $PV = nRT$?
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