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luckis11
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That 1 litre of hydrogen contains the same number of molecules with 1 litre of oxygen.
http://www.engineeringtoolbox.com/gas-density-d_158.htmlluckis11 said:Can you post links of this evidence? I have my doubts you see. E.g. when you say "1 litre of hydrogen" you mean that they let a particular weight of liquid hydrogen to evaporate in a box of 1 litre which contained vacaum, and also etc?
No, it is an experimental result. You weight a box (with known volume) with vacuum, and weight it filled with hydrogen at standard pressure and temperature, and calculate the difference. No liquids involved.luckis11 said:this density of hydrogen is derived by Avogadro΄s hypothesis?
That's why you compare it to a box with vacuum. Or, once you measured the density of air that way, you can subtract it via calculations.luckis11 said:because as this is a low density comparing to water΄s, I am not sure whether e.g. any surrounding buoyncy because of air is taking place
That would be equivalent to the chemical reaction suggested above. You always get twice the volume of hydrogen compared to the volume of oxygen in water electrolysis, for example.luckis11 said:THUS, something at electrolysis or counter-electrolysis can be the only proof I can think of.
luckis11 said:Can you post links of this evidence?
luckis11 said:if we have weight of 70 kilograms of liquid hydrogen in 1 metre^3 I am not sure that its mass i.e. the number of its noucleons is (70/1000) (the number of nucleons in 1000 kilograms of water)
.Scott said:http://www.engineeringtoolbox.com/gas-density-d_158.html
Note these STP densities:
[itex]O_2: 1.4290 kg/m^3 [/itex]
[itex]H_2: 0.0899 kg/m^3 [/itex]
And these molecualr weights:
[itex]O_2: 32.000 [/itex]
[itex]H_2: 2.016 [/itex]
Dividing through:
[itex]O_2: 1.4290 kg/m^3 / 32.000 = 0.0447 kg/m^3 [/itex]
[itex]H_2: 0.0899 kg/m^3 / 2.016 = 0.0446 kg/m^3 [/itex]
luckis11 said:Can you post links of this evidence? I have my doubts you see. E.g. when you say "1 litre of hydrogen" you mean that they let a particular weight of liquid hydrogen to evaporate in a box of 1 litre which contained vacaum, and also etc?
epenguin said:I think #2 and #4 for instance contain circular reasoning
luckis11 said:when you say "1 litre of hydrogen" you mean that they let a particular weight of liquid hydrogen to evaporate in a box of 1 litre which contained vacaum, and also etc?
One quotes atomic masses and the other a formula both assumed as known. How were they known? Originally via Avodgadro's hypothesis I think. At the start all anyone had was combining weights, so for Dalton water was HO, and the atomic mass of oxygen would have been 8.PeterDonis said:How so?
Right, but now we have mass spectrometry for a direct measurement.epenguin said:How were they known? Originally via Avodgadro's hypothesis I think.
epenguin said:At the start all anyone had was combining weights, so for Dalton water was HO, and the atomic mass of oxygen would have been 8.
mfb said:Right, but now we have mass spectrometry for a direct measurement.
Avogadro's law is a gas law that states that equal volumes of different gases, at the same temperature and pressure, contain the same number of molecules. It is also known as Avogadro's hypothesis or Avogadro's principle.
Avogadro's law was discovered by Amedeo Avogadro, an Italian scientist, in the early 19th century. However, his work was not recognized until many years later.
The proof for Avogadro's law comes from experimental data and mathematical equations. By conducting experiments with different gases and measuring their volumes, scientists were able to determine that equal volumes of different gases contain the same number of molecules when at the same temperature and pressure.
Avogadro's law is one of the fundamental principles that make up the ideal gas law. It states that at constant temperature and pressure, the volume of a gas is directly proportional to the number of molecules present. This relationship is expressed in the ideal gas law equation, PV = nRT, where n represents the number of moles of gas.
Avogadro's law is important because it helps us understand the behavior of gases and how they interact with each other. It also allows us to make predictions and calculations about gas behavior, which is crucial in various scientific and industrial applications such as in the production of food and medicines.