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Chemistry - Real Gas Question with Solution | TestHub

ChemistryReal GasLiquification & Critical Constants of GasesHard2 minQB

ChemistryHardnumerical

A van der Waals gas has $a = 3.64 L^{2}$ atm $m o l^{- 2}$ and $b = 42.7$ mL $m o l^{- 1}$ . Its critical pressure in atm (up to two decimal places) is

Answer:

73.94

Solution:

Convert $b = 42.7 m L / m o l = 0.0427 L / m o l$ .

Pc = $a / (27 b^{2}) = 3.64/ (27 \times 0.042 7^{2}) = 3.64/ (27 \times 0.001823) = 3.64/0.04923 = 73.94$ atm.

Trap: using $b = 42.7$ gives a value $1 0^{6}$ times too small.

Answer: 73.94.

Stream:JEESubject:ChemistryTopic:Real GasSubtopic:Liquification & Critical Constants of Gases

⏱ 2mℹ️ Source: QB

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