For one mole of a van der Waals gas when b = 0 and T = 300 K, the PV vs. 1 V plot is shown below. The value of the van der Waals constant a atm . litr e 2 mo l - 2 is

PV = ZRT and Z = 1 - a Z R T P V = 1 - a V R T R T PV = RT - a V Slope of graph between PV and 1 V is -a a = 21.6 - 20.1 3 - 2 = 1.5

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ChemistryReal GasMiscellaneous/MixedEasy2 minPYQ_2020

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For one mole of a van der Waals gas when b = 0 and T = 300 K, the PV vs. $\frac{1}{V}$ plot is shown below. The value of the van der Waals constant a $(atm . litr e^{2} mo l^{- 2})$ is

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Answer:

Solution:

$PV = ZRT$ and $Z = 1 - \frac{a}{Z R T}$

$P V = (1 - \frac{a}{V R T}) R T$

$PV = RT - \frac{a}{V}$

Slope of graph between PV and $\frac{1}{V}$ is -a

$a = \frac{21.6 - 20.1}{3 - 2} = 1.5$

Stream:NTA_ABHYASSubject:ChemistryTopic:Real GasSubtopic:Miscellaneous/Mixed

⏱ 2mℹ️ Source: PYQ_2020

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