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Liquefaction of Gases and Critical Constants

Which of the ...

Question

Which of the following statements about critical constants of gases are correct?

Larger

\frac{T_{c}}{P_{c}}

the value of a gas, larger would be the excluded volume

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Critical temperature

(T_{c})

of gas is greater than its Boyle's temperature

(T_{b})

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At the critical point in the van der Waal's gas isotherm

{(\frac{\partial P}{\partial V_{m}})}_{T_{c}} = 0

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V_{c} = 3 a

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Solution

The correct options are
B At the critical point in the van der Waal's gas isotherm ${(\frac{\partial P}{\partial V_{m}})}_{T_{c}} = 0$
D Larger $\frac{T_{c}}{P_{c}}$ the value of a gas, larger would be the excluded volume
Boyle's tempertaure of a gas is always higher than its critical temperature $(T_{c})$ . $T_{b} = \frac{a}{R_{b}}, T_{c} = \frac{8 a}{27 R_{b}}$
$V_{c} = 3 x b$

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Similar questions

Which of the following statements on critical constants of gases are correct?

I : Larger the $\frac{T_{c}}{P_{c}}$ value of a gas, larger would be the excluded volume.

II : Critical temperature ( $T_{c}$ ) of a gas is greater than its Boyle's temperature ( $T_{B}$ ).

III : At the critical point in the Van der Walls gas isotherm.

$⟮ \frac{d P}{d V_{m}} ⟯ T_{c} = 0$

I :

T_{c} / p_{c}

I I :

(T_{c})

(T_{b})

I I I :

(\frac{δ p}{δ V_{m}}) T_{c} = 0

T_{c}

\frac{T_{c}}{P_{c}}

P (V - b) = R T

[\frac{R}{V - b}]

H e

H_{2}

[\frac{T_{C}}{P_{C}}]

[\frac{T_{C}}{P_{C}}]

{(\frac{d P}{d V})}_{T_{C}} = 0

{(\frac{d P}{d V})}_{T_{C}} = 0

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