How much energy would be required to separate oxygen from carbon in a CO2 molecule?

Question

Just wondering. CO2 is covalent isn't it? How hard would it be to separate the oxygen and the carbon. Would introducing an electrical current help, or would that not aid it in any way? By the way, my grasp of chemistry is dodgy to say the least, incase you hadn't guessed.

Answer 1

The problem in separating the carbon and oxygen from CO2 is that CO2 is a VERY stable molecule, because of the bonds that hold the carbon and oxygen together, and it takes a lot of energy to separate them. Most schemes being considered now involve conversion to liquid or solids. One present concept for capturing CO2, such as from flue gases of boilers, involves chemical reaction with MEA (monoethanol amine). Other techniques include physical absorption; chemical reaction to methanol, polymers and copolymers, aromatic carboxylic acid, or urea; and reaction in plant photosynthetic systems (or synthetic versions thereof). Overcoming energetic hurdles is a major challenge; if the energy needed to drive these reactions comes from burning of fossil fuels, there may not be an overall gain. One aspect of the current research is the use of catalysts to promote the reactions. (In green plants, of course, chlorophyll is such a catalyst!) One area of current research is looking at using cellular components to imitate photosynthesis on an industrial scale.

Answer 2

Well in each molecule you need to break two C=O bonds. The energy required to do this can be found by looking in a data book/internet. Interestingly its the same amount of energy as you gain from burning one molecule of carbon (assuming the two oxygens bond once you have broken them off), but it will be applied less effeciently. So even if we achieved perfect energy transfers (which won't happen) doing this is rather pointless.

Answer 3

Water might nicely be chemically written as H2O. this implies it has 2 hydrogen atoms and one oxygen atom. there are a number of basic procedures to split the two. All contain very a good number of potential whilst in comparison with what you have consequently. severe warmth, electrical energy, severe warmth and electrical energy are all opportunities. the effect supply you H2 and additionally 0 to apply hydrogen as a gas you "burn" it it fairly is a physique of recommendations of oxidation. it is to declare you combine it with oxygen. whilst hydrogen (H2) burns the effect is H20 (water.) Water is an particularly stable substance. between the justifications that we've not got any loose hydrogen on earth is with the aid of the fact it desires to combine very effectively with oxygen which we've rather some in our environment. it fairly is not logical to not communicate of affordable or maybe useful to apply a gas it is confusing to get whilst there is an much less complicated determination. If we unexpectedly desperate we mandatory to get hydrogen we does not get it from water yet from organic gas (yet there could be pollution consequently.) it rather is plenty extra value effective and hence obtainable.

Answer 4

oh lord it's dodgy. to break the double bond would take a lot of energy. it's happy as CO2 and isn't coming apart unless you play with it

Answer 5

Electricity is the right direction, the effect your looking for is exactley what lighting does. This is how O3 is formed if i'm not mistaken.

Answer 6

You have to look up the exothermic and endothermic reactions in a special book which has the change over delta enthalpy or whatever in it.

Answer 7

It depends on how much CO2 you have. I think you maybe need a few types of tree, plants and algae, some sunlight, rain and a lot of time. :o)

Answer 8

a massive amount of energy. u cant so it from the mains socket

Answer 9

exactly 187 kcal/mole.

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