In the previous blogpost, we have discussed about the differences between Real Gas and Ideal Gas.
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Today, we shall look at why Different Real Gases deviate to a different extent from the Ideal Gas behaviour.
Recall from the Basic Assumptions of Kinetic Theory as applied to Ideal Gas, you will realised that Intermolecular Forces of Attraction plays a big part in the deviation of real gas from ideal gas behaviour.
Polar molecules have stronger forces of attraction between molecules and so, they will deviate much more from ideality as compared to non-polar molecules.
Example:
Let’s compare 3 gases (HCl, NH3 and H2) and see how we can apply the concepts we have just discussed:
This means that polar molecules such as NH3 and HCl (both are polar molecules) will deviate more from ideality as compared to H2 (non-polar molecule).
Further comparing NN3 and HCl, we will expect NH3 to deviate more than HCl from ideality due to Hydrogen-Bonding between NH3 molecules as compared to pd-pd forces between HCl molecules. (REVISE on the topic of Chemical Bondings)
As such, deviation from ideal gas behaviour increases as intermolecular forces increase.
H2 (weak id-id forces) < HCl (pd-pd) < NH3 (strong hydrogen-bonding)
Hope the above discussion is clear for your understanding.
In the next blog post, we will discuss on exam-based questions that are related to this concept.
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