Final answer:
The pressure of the air inside an inverted beaker would normally be equal to the atmospheric pressure if no other changes are made to the system. This pressure typically is around 1.00 atmosphere at sea level. Changes in temperature or volume of the air inside the beaker would alter the pressure according to Gay-Lussac's and Boyle's laws respectively.
Step-by-step explanation:
Air Pressure Inside an Inverted Beaker
The pressure of the air inside an inverted beaker would depend on the conditions set up in the experiment. If we are considering a normal laboratory situation where the beaker is simply flipped with air inside and no additional changes are made, then the pressure inside the beaker would be approximately equal to the surrounding atmospheric pressure. The air inside does not have an opportunity to expand or contract significantly, so its pressure remains close to 1.00 atmosphere (atm) which is the typical atmospheric pressure at sea level. At higher elevations, atmospheric pressure decreases, hence the pressure inside the beaker would, in such a case, also be lower.
Several factors could alter this simple scenario. For example, heating the air inside the beaker would raise its pressure according to Gay-Lussac's law, which says that pressure of a gas is directly proportional to its temperature when volume is held constant. Conversely, cooling the air would decrease its pressure. If the inverted beaker is part of an experiment involving changes in the volume of the trapped air, then Boyle's law would apply, which states that pressure is inversely proportional to volume for a given amount of gas at constant temperature.