At what temperature does carbon dioxide breaks up into oxygen and carbon?
820070
CO2 is a relatively stable compound and it would be very hard to thermally decompose it, although not impossible.  A quick internet search shows it can be done in precisely controlled environments using lasers (UV absorption to supply the required dissociation energy).  But there isn't really a cut and dry temperature.
481006
the boiling point of oxygen is -183oC.\n\nthe freezing point of carbon dioxide at atmospheric pressure is -78oC.\n\ntherefore having a mixture of the two in a flask, and cooling with liquid nitrogen (~-170oC) will freeze the CO2 to a solid, and leave the oxygen as a gas.  You can then separate the two.  If you feel -170oC is too close to the condensing point of oxygen, then add some diethyl ether to your liquid nitrogen and this will raise the temperature of your ice-bath to ~ -100oC.
768515
Very intense temparatures and pressures on Carbon.
685823
Strictly speaking, it is not true.  CO2, being heavier than air, WILL accumulate on ground level, if the air is perfectly still for a long enough period of time.  Or if the CO2 gas is colder than the air.  \n\nKeep in mind, though, that since the molecular weights of CO and of air are pretty close, the relative rate of diffusion of CO in air will be fairly slow.  That means if you have something making CO and putting it into the air, the worst place to be is right next to it.  Especially if the air is still.
115564
the temperature ranges from aprox. 50 kelvin to 53 kelvin.\nThat on the centigrate scale is -223 C to -220 C.
1175985
Balance the Carbons first, then the hydrogens, and lastly the oxygens:\nC3H8 + ?O2 --> 3CO2 + 4H2O\n(balances carbon and hydrogen)\nthen:\nC3H8 + 5O2 --> 3CO2 +4H2O (final answer)
489293
Good day! As far as I know CO2 or carbon dioxide does not destroy our atmosphere, as a matter of fact it's part of our atmosphere...The one that your telling that destroys our atmosphere is the CFC or Chlorofluorocarbon, that can be found in air fresheners, perfumes, air conditioners and refrigerators. And I read in a book that the destroyed part found in Australia can only be whole again if we pulverize all the seaweeds and distribute it up high(stratosphere). So, that's it, I hope I answered even a part of your question.
116688
from the equation: 2CO + O2 -----> 2CO2,\n\n0.69 g CO2 x (1 mol CO2/ 44 g CO2) x (2 mol CO/ 2 mol CO2) x (28 g CO/ 1 mol CO)\n\n\nthe answer is 0.4391 g of CO needs to react with O2 to produce 0.69 g of CO2
744972
It's easy. Just remember that carbon dioxide can dissolve in water to form carbonic acid. i.e. CO2(gas) + H2O(aqueous) => H2CO3 (aqueous)
454399
Yes, its called sublimation. It has to do with temperature and pressure. If you make CO2 (carbon dioxide) into a solid under really low temperatures and high pressure then when you take it out of the high pressure it will go directly into the gas phase.
642524
If you have a freezer that will lower the temp. of carbon dioxide to its freezing point you're straight in. Somewhere in the neighborhood of -125 Fahrenheit
447378
in biology, the exchange of carbon between living organisms and the nonliving environment. Inorganic carbon dioxide in the atmosphere is converted by plants into simple carbohydrates, which are then used to produce more complex substances. Animals eat the plants and are then eaten by other animals. When these life forms die, they decay, breaking down into, among many other things, carbon dioxide, which returns to the atmosphere. Plants and animals also release carbon dioxide during respiration. Animals and some microorganisms require the carbon-containing substances from plants in order to produce energy and as a source of materials for many of their own biochemical reactions; this cycle is vital to them. The process of incorporating carbon dioxide into the molecules of living matter is called fixation. Nearly all carbon dioxide fixation is accomplished by means of photosynthesis, in which green plants form carbohydrates from carbon dioxide and water, using the energy of sunlight to drive the chemical reactions involved. Green plants use carbohydrates to build the other organic molecules that make up their cells, such as cellulose, fats, proteins, and nucleic acids. Some of these compounds require the incorporation of nitrogen (see nitrogen cycle). When carbohydrates are oxidized in cells they release the energy stored in their chemical bonds, and some of that energy is also used by the cell to drive other reactions. In the process of oxidation, or respiration, oxygen from the atmosphere (or from water) is combined with portions of the carbohydrate molecule, producing carbon dioxide and water, the compounds from which the carbohydrates were originally formed. However, not all of the carbon atoms incorporated by the plant can be returned to the atmosphere by its own respiration; some remain fixed in the organic materials that make up its cells. When the plant dies, its tissues are consumed by bacteria and other microorganisms, a process called decay. These microorganisms break down the organic molecules of the plant and use them for their own cell-building and energy needs; by their respiration more of the carbon is returned to the atmosphere. The carbon-containing molecules that an animal derives from consuming other organisms are reorganized to build its own cells or oxidized for energy by respiration, releasing carbon dioxide and water. When the animal dies it too is decayed by microorganisms, resulting in the return of more carbon to the atmosphere. Carbon-containing molecules in wood (or other dry, slow-decaying organic materials) may be oxidized by burning, or combustion, also producing carbon dioxide and water. Under conditions prevailing on earth at certain times, green plants have decayed only partially and have been transformed into fossil fuels–coal, peat, and oil. These materials are made of organic compounds formed by the plants; when burned, they too restore carbon dioxide to the atmosphere.
725482
rapid expansion of CO2 gas in the cylinder to CO2 in the atmosphere greatly reduces the gas temperature. this is the reverse of gas compression, in which compression of a gas increases its temperature.\n\nan expanding gas does work on the surrounding, this energy comes from its own kinetic energy, which is analogous to its absolute temperature. the more a gas expands, the more energy it uses and the lower its temperature becomes.
813754
O2, N2 and CO2.\n\nDon't understand the last part
754768
Carbon at room temperature and pressure is a solid, not a gas. If you raised its temperature enough to make it a gas, it would become highly reactive and would be too hot for you to breathe.
202502
The answer is very basic. Start with chemical names.  Carbon dioxide is made from carbon and oxygen. Carbon is called C, and Oxygen is called O. If you have two atoms of O, and one atom of C, then you have Carbon dioxide. The shorthand notaion for this is CO2. Don't be afraid of chemical formulas, but bring yourself to be comfortable with them, so you don't freak when you have to do a problem like this:\n__H4C + __O4Fe---->__HCO + __Fe. (this is balancing equations, but they're easy, once you learn to decode what chemical equations are trying to tell you )\n\nOn this website, just look at the ones that are relevant:\nhttp://www.ukrocketry.co.uk/forum/index.php?s=e26325e497d951d76619a79a0ad64ae7&showtopic=381\n\n\n\n\n\nThis si a segment on this from my school textbook: (sorry, its kinda long)\nA molecule or compound consists of at least two atoms that are chemically bonded. The chemical formula of a molecule or compound states how many atoms of each element are in one of its molecules. This formula is similar to an algebraic formula in its use of symbols. The description of a compound with numbers and symbols is called a chemical formula. Some formulae can be quite complex.\n\nQuestions you may have are:\n\nWhat are chemical compounds? \nWhat is the numbering system in a chemical formula? \nHow do you designate complex compounds? \nThis lesson will explain the basics of chemical formulas. \n\nChemical compounds\nA molecule is the chemical combination of two or more atoms. They can be of the same element, such as in the oxygen molecule (O2) or different as in the water molecule (H2O)\n\nA compound is a molecule that is made up of at least two different elements. The water molecule is a compound. When atoms of different elements combine to form a compound, the result is a new substance that has different properties than the original elements. A good example is when the poisonous green chlorine gas is combined with the explosive metal sodium to form the white salt crystals we use in our food.\n\nThe study of Chemistry is mainly interested in the formation of chemical compounds, since there are so many possible combinations of elements.\n\nChemical formulas\nChemical formulas (or more correctly: formulae) are designations of molecules and compounds in shorthand notation, similar to that used in Algebra.\n\nElements can be written as abbreviations or in a shorthand notation. For example, He denotes helium, Fe denotes iron, and Cl denotes chlorine. A chemical formula is writing the elements of a compound, using their abbreviations.\n\nThe combination of two or more elements to form a molecule is designated by writing their abbreviations next to each other. For example carbon monoxide is written as CO. The order in which the elements are written is typically alphabetical, but there are a number of exceptions for historical reasons and to clarify the geometry of the molecule.\n\nIf there is more than one atom of a type in the molecule, the formula shows it by a small number after the symbol. For example, water is H2O, which means there are 2 atoms of hydrogen and one atom of oxygen in the molecule. Carbon dioxide is CO2, which means there is one atom of carbon and two atoms of oxygen in the molecule.\n\nTo show the number of molecules, a full sized number is located in front of the molecule. For example 4 molecules of carbon dioxide is designated as:\n\n4CO2\n\nThis means there are a total of 4 C atoms and 8 O atoms in the combination. A way to remember this—taken from Algebra—is to think of it as 4 x (CO2).\n\nComplex formulae\nJust as in Algebra, you can use parentheses to separate parts in a complex formula. One example is the formula for nitroglycerin, a highly explosive substance.\n\nC3H5(NO3)3\n\nThis formula shows that nitroglycerin consists of 3 atoms of C, 5 atoms of H and then 3 molecules of NO3. If the parentheses were not used, you might have a formula like:\n\nC3H5N3O9\n\nThe number of atoms for each el
904836
carbon dioxide from the air combining with ribulose 1,5 bisphosphate