Under what conditions do real gases behave as ideal gases?
- AHigh pressure and low temperature
- BLow pressure and high temperature
- CHigh pressure and high temperature
- DLow pressure and low temperature
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Assertion : Greater the value of van der Waal's constant $a$,greater is the liquefaction of gas.
Reason : $a$ indirectly measures the magnitude of attractive forces between the molecules.
Reason : $a$ indirectly measures the magnitude of attractive forces between the molecules.
The cooling in a refrigerator is due to
Easy
View SolutionIf the compressibility factor $(Z)$ of a real gas is $1.05$ at $STP$,what is the molar volume of the real gas (in $dm^3$)?
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 unit of the van der Waals gas equation parameter $a$ in $(P + \frac{an^{2}}{V^{2}})(V - nb) = nRT$ is :
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