It was first stated by Émile Clapeyron in 1834 as a combination of Boyle's law and Charles's law. It was first stated by Émile Clapeyron in 1834 as a combination of Boyle's law and Charles's law.
Charles Law is the name of the experimental gas law which states that when a gas is heated under constant pressure, there is a proportional increase in volume or in other words
V1/T1=V2/T2
Where V1 and V2 are the initial and final volumes and T1 and T2 are the final and initial temperatures. The law was first published by a French philosopher by the name of Joseph Louis Gay-Lussac in 1802, but he claimed that Jacques Charles had already discovered it in the 1780s and thus used Charles' name instead of his own. However, a British philosopher by the name of John Dalton independent discovered it on his own in 1801, but his work was not as thorough as Gay-Lussac's. In addition, the basics had been discovered nearly a century earlier by another French scientist, Guillaume Amontons, but his work was even more basic.
While mostly accurate, this equation is but an estimate of a much more complicated law. This equation makes many assumptions about gas particles that are not true that will cause small but noticeable deviations from values as expected. A Dutch physicist by the name of Johannes Diderik van der Waals updated the law in 1873 to account for these imperfections and is still an accurate description to this day.
by Irish Scientist Robert Boyle by Irish Scientist Robert Boyle by Irish Scientist Robert Boyle
i think Michael boltzmann did, he's the one who came up w/ the entropy equation for the chaos w/ the gas particles S=klogW
haha yu needa find the anwser yur self stop lookin for anwsers
This chemist was Emile Clapeyron.
Boyle.
What does the ideal gas law not specify the density and mass of the gas. It instead deals with volume, temperature and pressure.
The ideal gas law: PV=nRT Where n=the number of moles
The ideal gas law
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.
Not true. It applies to real gases that are exhibiting ideal behavior. Any gas that is not 'close' to its boiling and is at a 'low' pressure will behave like an ideal gas and Boyle's Law can be applied. Remember there is no such thing as an ideal gas, so when Boyle did his experiments and came up with his law he was using a real gas, probably just air.
All gas laws are absolutely accurate only for an ideal gas.
the ideal gas constant D:
Charles' Law and other observations of gases are incorporated into the Ideal Gas Law. The Ideal Gas Law states that in an ideal gas the relationship between pressure, volume, temperature, and mass as PV = nRT, where P is pressure, V is volume, n is the number of moles (a measure of mass), R is the gas constant, and T is temperature. While this law specifically applies to ideal gases, most gases approximate the Ideal Gas Law under most conditions. Of particular note is the inclusion of density (mass and volume) and temperature, indicating a relationship between these three properties.The relationship between the pressure, volume, temperature, and amount of a gas ~APEX
What does the ideal gas law not specify the density and mass of the gas. It instead deals with volume, temperature and pressure.
This is the general ideal gas law.
Pressure is given as pascals in the ideal gas equation.
Ideal gas law states that there are no inter molecular attractions between gas molecules and that ideal gas does not occupy space therefore having no volume. However, a real gas does have intermolecular attractions and does have a volume.
The ideal gas law does not hold that gasses are massless. Gas does indeed have mass. Saturn has a mass of about 5.68*1026 kilograms.
The ideal gas law is:PV = nRT,where:- P is pressure- V is volume- n is moles of substance- R is the gas constant- T is the temperature
If gas molecules were true geometric points (ie had zero volume) AND had zero intermolecular interaction (such as attraction or repulsion), then the gas would obey the ideal gas law. Gases composed of small, non-interactive molecules (such as helium gas) obey the ideal gas law pretty well (as long as the gas is low density and temperature is rather high). For non-ideal gases, at least two correction factors are often used to modify the ideal gas law (correcting for non-zero volume of gas molecule and intermolecular attraction) such as in the Van der Waals equation for a real gas.
atmospheres A+
The ideal gas law: PV=nRT Where n=the number of moles