Consider the equation $Z = \frac{PV}{RT}.$ Which of the following statements is correct?
- AWhen $Z > 1,$ real gases are easier to compress than the ideal gas
- BWhen $Z > 1,$ real gases show negative deviation
- CWhen $Z > 1,$ real gases are difficult to compress
- DNone of these
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Similar Questions
Consider the van der Waals constants,$a$ and $b$,for the following gases:
Gas $Ar$ $Ne$ $Kr$ $Xe$ $a / (atm \ dm^6 \ mol^{-2})$ $1.3$ $0.2$ $5.1$ $4.1$ $b / (10^{-2} \ dm^3 \ mol^{-1})$ $3.2$ $1.7$ $1.0$ $5.0$
Which gas is expected to have the highest critical temperature?
| Gas | $Ar$ | $Ne$ | $Kr$ | $Xe$ |
|---|---|---|---|---|
| $a / (atm \ dm^6 \ mol^{-2})$ | $1.3$ | $0.2$ | $5.1$ | $4.1$ |
| $b / (10^{-2} \ dm^3 \ mol^{-1})$ | $3.2$ | $1.7$ | $1.0$ | $5.0$ |
Which gas is expected to have the highest critical temperature?
MediumAIIMS 2019
View SolutionWhen is deviation more in the behaviour of a gas from the ideal gas equation $PV = nRT$?
$A$ gas deviates most from ideal behavior when it is subjected to
Positive deviation from ideal behaviour is due to the fact that
Easy
View SolutionWhich gas shows real behavior?
Medium
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