KCET · Chemistry · Alcohols Phenols and Ethers
The pressure of real gases is less than that of ideal gas because of
- A Intermolecular attraction
- B Finite size of particles
- C Increase in the number of collisions
- D Increase in the kinetic energy of the molecules
Answer & Solution
Correct Answer
(A) Intermolecular attraction
Step-by-step Solution
Detailed explanation
The force of attraction in real gases tend to show slightly lower pressure as compared to ideal gasses.
\( p_{\text {ideal }}=p_{\text {real }}+\frac{a n^{2}}{V^{2}} \) or \( p_{\text {real }}=p_{\text {ideal }}-\frac{a n^{2}}{V^{2}} \)
where ' \( \mathrm{a} \) ' is the constant which measure the magnitude of attractive forces among the molecules of gas ' \( \mathrm{n} \) ' is the no. of
moles present and ' \( V^{\prime} \) is the volume of gas present.
\( p_{\text {ideal }}=p_{\text {real }}+\frac{a n^{2}}{V^{2}} \) or \( p_{\text {real }}=p_{\text {ideal }}-\frac{a n^{2}}{V^{2}} \)
where ' \( \mathrm{a} \) ' is the constant which measure the magnitude of attractive forces among the molecules of gas ' \( \mathrm{n} \) ' is the no. of
moles present and ' \( V^{\prime} \) is the volume of gas present.
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