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              Consider the following table :

Gas           a/(k\: \: Pa \: \: dm^{6}\: \: mol^{-1})        b/(\: \: dm^{3}\: \: mol^{-1})

A                           642.32                                      0.05196

B                          155.21                                       0.04136

C                          431.91                                       0.05196

D                          155.21                                       0.4382

               a and b are van der Waals constants. The correct statement about the gases is :

  • Option 1)

    Gas C will occupy more volume than gas A;

    gas B will be more compressible than gas D

  • Option 2)

    Gas C will occupy lesser volume than gas A;

    gas B will be lesser compressible than gas D

  • Option 3)

    Gas C will occupy more volume than gas A;

    gas B will be lesser compressible than gas D

  • Option 4)

    Gas C will occupy lesser volume than gas A;

    gas B will be more compressible than gas D

Answers (3)

best_answer

In Vanderwaal's equation,

[P+a(\frac{n}{V})^{2}](\frac{V}{n}-b)=RT

a & b are constants     

Here 'a' is defined as greater the value of 'a' ,

greater is the force of attraction & smaller is the volume.

& ' b ' is defined the greater the value of ' b ' , higher will 

be the effective volume & less will be the compressibility.

\therefore  Gas 'C' will occupy more volume than Gas 'A' , Gas 'B'

will be more compressible than Gas 'D'.

\therefore option (1) is correct.

 


Option 1)

Gas C will occupy more volume than gas A;

gas B will be more compressible than gas D

Option 2)

Gas C will occupy lesser volume than gas A;

gas B will be lesser compressible than gas D

Option 3)

Gas C will occupy more volume than gas A;

gas B will be lesser compressible than gas D

Option 4)

Gas C will occupy lesser volume than gas A;

gas B will be more compressible than gas D

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solutionqc

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