An ideal gas as compared to a real gas at very high
pressure occupies
(a) more volume (b) less volume
(c) same volume
(d) unpredictable behaviour
(e) no such correlation.
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Answer:
An ‘ideal gas’ as compared to the real gas at ‘very high pressure’ which occupies “more volume”.
Explanation:
- The reason for ideal gas occupying more volume is well explained by ideal gas law, assuming that the masses are points which takes up no volume.
- The real molecule takes some of the volume and at high pressure the fraction of this becomes more significant.
- That means that every molecules travel a very short distance between the collisions.
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