Consider the following table:

Gas $a (k P a d m^{6} m o l^{- 2})$ $b (d m^{3} m o l^{- 1})$

A 642.32 0.05196

B 155.21 0.04136

C 431.91 0.05196

D 155.21 0.4382

a and b are vander waals constant. The correct statement about the gases is:

Gas C will ocupy lesser volume than gas A; gas B will be lesser compressible than gas D

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Gas C will occupy more volume than gas A; gas B will be lesser compressible than gas D

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Gas C will occupy more volume than gas A; gas B will be more compressible than gas D

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Gas C will occupy lesser volume than gas A; gas B will be more compressible than gas D

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Solution

The correct option is C Gas C will occupy more volume than gas A; gas B will be more compressible than gas D
Gas C will occupy more volume than gas A; gas B will be more compressible than gas D.
Gas A and C have same value of 'b' but different value of 'a' so gas having higher value of 'a' have more force of attraction so molecules will be more closer hence occupy less volume.
Gas B and D have same value of 'a' but different value of 'b' so gas having lesser value of 'b' will be more compressible.

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Similar questions

A, B

C

\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}

a / d m^{6} k P a m o l^{- 2}

b / d m^{3} m o l^{- 1}

^{'} a^{'}

H C l

371.843 K P a

b = 40.8 c m^{3} m o l^{- 1}

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}

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