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is c02 heavier than air

Incidentally, if you cooled these gasses down and pressurized them until they liquified (liquid oxygen is used as rocket fuel, liquid carbon dioxide is used to carbonate soft drinks) you would get a different answer. Liquid oxygen is actually heavier than liquid carbon dioxide by a little bit. 1.149 grams/ milliliter for liquid oxygen at its boiling point versus 1.101 grams/ milliliter for liquid carbon dioxide.
If you cool even more and get solid oxygen and carbon dioxide you would find than carbon dioxide is slightly heavier than a similar volume of solid oxygen. Solid carbon dioxide is also known as dry ice, and is used to keep thing cold when ordinary ice is not good enough.
At room temperature and atmospheric pressure, oxygen and carbon dioxide are both gasses. In fact, they are close to what scientists call ideal gasses. Ideal gasses are much more easy to understand than non-ideal gasses. For ideal gasses, the density of the gas (the weight for a given volume–basically the heaviness) is directly proportional to the mass of an individual molecule. For oxygen, a molecule consists of two oxygen atoms, and has a weight of 2 x 16 = 32. For carbon dioxide, there is one carbon atom (weight 12) and two oxygen atoms (mass 16 x 2) for a total of 44. This means that carbon dioxide should be about 44/32 = 1.375 times as heavy as an equivalent volume of oxygen. In reality, oxygen gas has a density of 1.429 grams/liter at the so-called standard pressure and temperature (basically room temperature and atmospheric pressure) while carbon dioxide has a density of 1.977 grams/liter. If you do the math, you will find that carbon dioxide is 1.383 times as heavy as oxygen. This means that the “ideal gas model” is very good in this case.
If you’ve ever seen the smoke that comes off of dry ice, you probably already knew the answer to your question, as that “smoke” is actually carbon dioxide gas mixed with water vapor, and tends to “sink” and collect on the floor or on counter tops until it mixes with the air and disperses.
That is an interesting question. Once, when I was at the Exploratorium, a science museum in San Francisco, I saw a great exhibit that actually answered your question perfectly! The exhibit had you blow a single soap bubble into a large tub with dry ice at the bottom. The soap bubble sank towards the bottom of the tub at first, as you would expect, but instead of hitting the bottom and popping, the bubble gradually stopped falling and finally sat suspended in the air! Dry ice gives off carbon dioxide gas, and so there was a thick layer of carbon dioxide in the bottom of the tub. Because carbon dioxide is heavier than air, and the bubble was made of air, the bubble actually floated above the carbon dioxide layer because it was lighter. Eventually, the chill from the dry ice froze the soap on the surface of the bubble and the bubble sank to the bottom of the tub and stayed there, a perfect sphere of hollow ice.
What you are really interested in the density of the gas, rather than the weight.For most gases at atmospheric pressure, a given volume contains the same number of molecules at a given temperature. This is known as the ideal gas law. The density (or how “heavy”) something is depends on the amount of mass per volume – a pound of lead and a pound of feathers has the same mass, but take up quite different volumes, and hence have quite different densities, with the leak having a high density (heavy) and the feathers having a low density (light). For an ideal gas, the density is just the molecular weight of the gas, divided by the volume of a given number of molecules. Since a given number of molecules always takes up the same volume for a gas, the higher the molecular weight, the “heavier” the gas is, or the higher the density. Carbon dioxide has one carbon atom and two oxygen atoms, and a molecular weight of 44 grams per mole ( a certain number of molecules). The oxygen in the air is actually O2, or molecular oxygen, with a molecular weight of 32. Hence, carbon dioxide has a higher density, or is heavier than oxygen. That is why you need to be careful with carbon dioxide. It can displace the oxygen in a room and lead to asphyxiation.
I’ll give you a hint on this one and then I bet you’ll be able to figure it out for yourselves. The symbol for oxygen is O and the symbol for carbon dioxide is CO2.
Carbon has an atomic wt of 12, oxygen in diatomic form(O2) of 32 and CO2 of 44. this means that the mass of 6×10 23 atoms of CARBON has a mass of 6 kilograms, the mass of 6×10 23 diatomic oxygen molecules is 32 kg, and for CO2 its 44kg, so carbon is the lightest and CO2 the heaviest.
So one mole of O2 weights : 2 x 16 = 32 grams
Is c02 heavier than air At room temperature and atmospheric pressure, oxygen and carbon dioxide are both gasses. In fact, they are close to what scientists call ideal gasses. Ideal gasses are
Is c02 heavier than air
October 25, 2019 at 2:46 pm | #
“If CO2 didn’t mix with non-CO2 fast, you wouldn’t be able to lie on your stomach without suffocating, since your breath is 38K ppm or higher CO2, and the lethal concentration starts at about 50K ppm”
October 26, 2019 at 3:05 am | #
October 27, 2019 at 3:09 pm | #
Hi Jerry,
No doubt thunderstorm N2 adds to the fertilising benefits. CO2 will always combine with atmospheric moisture to the extent quoted, regardless of thunderstorm activity. I wonder how much of these fertilising agents are removed during the water treatment process?
October 26, 2019 at 11:36 am | #
Written by TL Winslow
Trap heat as a greenhouse gas? Sorry, being thoroughly mixed with non-CO2 molecules, every time a CO2 molecule gets hotter than its neighbors, they sap the extra heat to equalize temperatures. The air as a whole conducts solar heat at Earth’s surface and convects it towards space, and CO2 is just trapped in the rest of the air and goes along with it. Hence the Earth’s atmosphere is not a greenhouse but a giant chimney, and all the elaborate claims of CO2 greenhouse warming theory are moose hockey.
October 28, 2019 at 11:09 am | #
CO2 is a gas, which is like a collection of zillions of hard bouncy balls whose kinetic energy comes from the overall temperature.