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What would be the pressure theoretically at absolute zero?
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What pressure would you expect in a rigid container of 0 centigrade gas if you cooled it by 273 centigrade?
If you cool the container to -273 degrees Celsius, which is absolute zero, the gas would theoretically have zero pressure since all molecular motion would cease. In practice, achieving absolute zero is impossible, but as you approach it, pressure would approach zero.
What is the zero point on the absolute scale defined as?
SZero point in the absolute scale is the temperature at which the kinetic energy of the molecule becomes Zero. For a constant pressure volume would become zero and at constant volume pressure would become zero at this absolute zero temperature.
If a certain amount of gas fills a 1.0 liter container and exerts a pressure on the walls of 2.0 Nm2 at 20 degrees celsius what would the pressure theoretically be at absolute zero?
Zero. PV = nRT. T = 0, so nRT = 0, and thus PV must be zero also. Since we know the volume is not zero, the pressure must be zero.
Would you have obtained a different temperature for absolute zero if you recorded the pressure in psi instead of kpa?
No, the temperature for absolute zero would remain the same regardless of whether pressure is recorded in psi or kPa. Absolute zero is defined as 0 Kelvin, which corresponds to a theoretical temperature where molecular motion ceases. While pressure measurements in different units may yield different numerical values, they do not affect the fundamental physical properties of temperature and absolute zero.
Would you consider atmospheric pressure when finding the pressure of a liquid in a closed container?
pressure is usually measured relative to atmospheric this is called gauge pressure. if you compare against absolute zero pressure (vacuum) this is called absolute pressure.
Why would the pressure be 0 for absolutle zero?
The pressure of a gas is exerted on the walls of its container by the movement of the molecules making up the gas. The higher the temperature, the faster the particles move, increasing the pressure exerted on the sides of the container. As the temperature decreases, the movement of the gas particles slows down, reducing the pressure. At absolute zero, the gas particles would be completely frozen so that no particles would be hitting the sides of the container and the pressure exerted by the gas would be zero. This is all theoretical since absolute zero cannot yet be reached, and gas would not actually be able to have a pressure of zero.
What would the volume and pressure of an ideal gas be at absolute zero temperature IF an ideal gas actually existed?
Here's the ideal gas law: PV = nRT If T is zero, then PV must be zero; assuming the volume is nonzero, then for PV to be zero the pressure must be zero. However, this is only true for an ideal gas. For a real gas other factors come into play at low temperatures, and they begin to deviate from the ideal gas law. Also, all real gases liquify above absolute zero, and liquids don't obey the ideal gas law at all.
Is it possible for absolute pressure to be negative?
No, absolute pressure cannot be negative as it is always measured as a positive value above zero.
What is the temperature at which an ideal gas occupies zero pressure?
The temperature at which an ideal gas occupies zero pressure is called absolute zero. It is defined as 0 Kelvin or -273.15 degrees Celsius. At this temperature, the particles in the gas have minimal kinetic energy and do not exert any pressure.
What is significant about the temperature absolute zero?
The most significant thing about the temperature of absolute zero is that is marks the point where molecular motion stops. It is equal to −459.67 degrees Fahrenheit.
What is the volume of an ideal gas at absolute zero temperature?
At absolute zero temperature, the volume of an ideal gas would theoretically be zero.
