(A) The Van der Waals equation is given by $\left( P + \frac{n^2a}{V^2} \right)(V - nb) = nRT$.At low pressure,the volume $V$ is very large,making the

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temperature is sufficiently high and pressure is low

(A) The Van der Waals equation is given by $\left( P + \frac{n^2a}{V^2} \right)(V - nb) = nRT$.At low pressure,the volume $V$ is very large,making the correction term $\frac{n^2a}{V^2}$ negligible compared to $P$.At high temperature,the volume $V$ is also large,making the correction term $nb$ negligible compared to $V$.Under these conditions,the equation simplifies to $PV = nRT$,which is the ideal gas equation.

Class 11 Chemistry States of Matter Real gases and Vander waal’s equation

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Van der Waals equation for a gas is stated as,
$p = \frac{nRT}{V - nb} - a\left( \frac{n}{V} \right)^2$
This equation reduces to the perfect gas equation,$p = \frac{nRT}{V}$,when:

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A
temperature is sufficiently high and pressure is low
B
temperature is sufficiently low and pressure is high
C
both temperature and pressure are very high
D
both temperature and pressure are very low

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Real gases and Vander waal’s equation

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The graph between $P$ and $V$ below the critical temperature is:

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What kind of deviation will $2 \, mol$ of $N_2$ gas show in a $50 \, L$ container at $STP$?

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Under which of the following conditions does a gas deviate from ideal behaviour?
$A$. Low pressure
$B$. High pressure
$C$. Low temperature
$D$. High temperature

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Which of the following statements is false based on the provided graph of compressibility factor $Z$ versus pressure $P$?

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The given graph represents the variation of $Z$ (compressibility factor = $\frac{PV}{nRT}$) versus $P$,for three real gases $A, B$ and $C$. Identify the only incorrect statement.

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Van der Waals equation for a gas is stated as,$p = \frac{nRT}{V - nb} - a\left( \frac{n}{V} \right)^2$This equation reduces to the perfect gas equation,$p = \frac{nRT}{V}$,when:

Similar Questions

The graph between $P$ and $V$ below the critical temperature is:

What kind of deviation will $2 \, mol$ of $N_2$ gas show in a $50 \, L$ container at $STP$?

Under which of the following conditions does a gas deviate from ideal behaviour?$A$. Low pressure$B$. High pressure$C$. Low temperature$D$. High temperature

Which of the following statements is false based on the provided graph of compressibility factor $Z$ versus pressure $P$?

The given graph represents the variation of $Z$ (compressibility factor = $\frac{PV}{nRT}$) versus $P$,for three real gases $A, B$ and $C$. Identify the only incorrect statement.

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Van der Waals equation for a gas is stated as,
$p = \frac{nRT}{V - nb} - a\left( \frac{n}{V} \right)^2$
This equation reduces to the perfect gas equation,$p = \frac{nRT}{V}$,when:

Under which of the following conditions does a gas deviate from ideal behaviour?
$A$. Low pressure
$B$. High pressure
$C$. Low temperature
$D$. High temperature