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Byju's Answer

Standard XII

Chemistry

System, Surroundings, Intensive, Extensive Properties

If the van de...

Question

If the van der waals parameters of two gases are given as:
$a - d m^{6} b a r m o l^{- 2} b - d m^{3} b a r m o l^{- 1}$
$\begin{matrix} G a s A - 6.5 & 0.056 G a s B - 18.0 & 0.011 \end{matrix}$
Then which of the above statements is / are correct?

Critical presssure of A< critical pressure of B.

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Critical temperature of A< critical temperature of B.

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Both a and b

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None of the above

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Solution

The correct option is C Both a and b
As we know,
$V_{c} = 3 b, T_{c} = \frac{8 a}{27 R b^{'}} P_{c} = \frac{a}{27 b^{2}}$
For critical volume,
Since, $b_{A} > b_{B} \Rightarrow V_{c (A)} > V_{c (B)}$
Since ${(\frac{a}{b})}_{A} < {(\frac{a}{b})}_{B} \Rightarrow T_{c (A)} < T_{c (B)}$
For Critical temperature -
Since, ${(\frac{a}{b})}_{A} < {(\frac{a}{b})}_{B} \Rightarrow T_{c (A)} < T_{c (B)}$
Option B is correct
For critical pressure-
${(\frac{a}{b^{2}})}_{A} < {(\frac{a}{b^{2}})}_{B} \Rightarrow P_{c (A)} < P_{c (B)}$

Suggest Corrections

Similar questions

Q. If the van der waals parameters of two gases are given as:

a - d m^{6} b a r m o l^{- 2} b - d m^{3} b a r m o l^{- 1}

\begin{matrix} G a s A - 6.5 & 0.056 G a s B - 18.0 & 0.011 \end{matrix}

Then which of the above statements is / are correct?

Q. The vander waals constant for gases

A, B

and

C

are as follows:

\begin{matrix} Gas & {a/dm}^{6} {kPa mol}^{- 2} & {b/dm}^{3} {mol}^{- 1} A & 405.3 & 0.027 B & 1215.9 & 0.030 C & 607.95 & 0.032 \end{matrix}

Which gas has highest critical temperature :

The essential conditions for liquefaction of gases were discovered by Andrews in

1869

as a result of his study of pressure-volume-temperature relationship for

C O_{2}

. It was found that above a certain temperature, it was impossible to liquefy a gas whatever the pressure was applied. The temperature below which the gas can be liquefied by the application of pressure alone is called critical temperature

(T_{c})

. The pressure required to liquefy a gas at this temperature is called the critical pressure

(P_{c)}

. The volume occupied by one mole of the substance at the critical temperature and pressure is called critical volume. Critical constants are related with van der Waals' constant as follows:

V_{c} = 3 b, P_{c} = \frac{a}{27 b^{2}}, T_{c} = \frac{8 a}{27 R b}

Which of the following parameters is three times the van der Waals' constant

^{'} b^{'}

Q. The van der Waals parameters for gases

W, X, Y

and

Z

are:

\begin{matrix} G a s & a (a t m L^{2} m o l^{- 2}) & b (L M o l^{- 1}) W & 4.0 & 0.027 X & 8.0 & 0.030 Y & 6.0 & 0.032 Z & 12.0 & 0.027 \end{matrix}

Which one of these gases has the lowest critical temperature?

The van der Waals' parameters for gases W,X,Y and Z are

$\begin{matrix} G a s & a (l i t r e^{2} - a t o m / m o l^{2}) & b (l i t r e / m o l) W & 4.0 & 0.027 X & 8.0 & 0.030 Y & 6.0 & 0.032 Z & 12.0 & 0.027 \end{matrix}$

Which one of these gases has the highest critical temperature?

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If the van der waals parameters of two gases are given as: a−dm6bar mol−2 b−dm3bar mol−1 GasA−6.50.056GasB−18.00.011 Then which of the above statements is / are correct?

The correct option is C Both a and bAs we know, Vc=3b,Tc=8a27Rb′Pc=a27b2 For critical volume, Since, bA>bB⇒Vc(A)>Vc(B) Since (ab)A<(ab)B⇒Tc(A)<Tc(B) For Critical temperature - Since, (ab)A<(ab)B⇒Tc(A)<Tc(B) Option B is correct For critical pressure- (ab2)A<(ab2)B⇒Pc(A)<Pc(B)

If the van der waals parameters of two gases are given as:
$a - d m^{6} b a r m o l^{- 2} b - d m^{3} b a r m o l^{- 1}$
$\begin{matrix} G a s A - 6.5 & 0.056 G a s B - 18.0 & 0.011 \end{matrix}$
Then which of the above statements is / are correct?