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Kiara
- 14
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If I know that liquid helium at 4.2 K (boiling point) occupies 0.01065 L, then how do I calculate the pressure exerted on the walls of its containers if the helium evaporates and warms up to 30 K?
The ending pressure of Helium gas can vary depending on several factors such as temperature, volume, and initial pressure. However, at standard temperature and pressure (STP), the ending pressure of Helium gas is about 1 atmosphere or 101.3 kilopascals.
The ending pressure of Helium gas can be determined using the ideal gas law, which states that the pressure of a gas is directly proportional to its temperature and inversely proportional to its volume. Other factors such as the number of moles and the gas constant also play a role in determining the ending pressure.
According to the ideal gas law, when the temperature of Helium gas increases, its ending pressure also increases. This is because the gas molecules gain more kinetic energy and move around faster, creating more collisions with the walls of the container and thus increasing the pressure.
No, the ending pressure of Helium gas cannot be negative. According to the ideal gas law, pressure is always a positive value and cannot be less than zero. If the pressure of Helium gas were to become negative, it would mean that the molecules are exerting a force pulling them inward instead of outward, which is not possible.
The ending pressure of Helium gas is generally lower than other gases at the same temperature and volume. This is because Helium gas has a lower molecular weight and thus its molecules move around faster, resulting in fewer collisions with the container walls and a lower pressure. However, at low temperatures and high pressures, Helium gas can behave similarly to other gases and have a higher ending pressure.