At a very high pressure, the volume of occupied by a real gas is greater than the volume predicted by the ideal gas law, because the volume of the actual particles is more significant under high pressure.
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Behavior of gases at low pressure and high pressures</h3>
At low pressure, the distance between gas molecules is relatively far apart, but as the pressure of the gas increases, the distances between theses gaseous molecules becomes smaller.
Due to the high pressure the volume occupied by the gas molecules becomes significant compared with the volume of the container.
As a result, the total volume occupied by the gas will be greater than the volume predicted by the ideal gas law.
Thus at a very high pressure, the volume of occupied by a real gas is greater than the volume predicted by the ideal gas law, because the volume of the actual particles is more significant under high pressure.
Learn more about behavior gases under pressure here: brainly.com/question/13512523
Answer:
5000 molecules of A will needed to react with 5000 molecules of B to gives 5000 molecules of AB.
Explanation:
A+B → AB
Given that 100 molecules of A combines with 100 molecules of B to give 100 molecules of AB.
According to reaction, 1 molecule of AB is produced by 1 molecule of A.
Then 5000 molecules of AB will be given by:
molecules of A
5000 molecules of A will needed to react with 5000 molecules of B to gives 5000 molecules of AB.
Conventional volcanoes are known to erupt after pressure builds up from new magma flowing into the magma chambers that lie below the vents on the Earth's surface.