what is atomic weight of CO2?
87793
44.00995 grams per mole
599859
It can vary, based on the conditions. However, according to Harris's Quantitative Analysis (2002), it's 4.69*10^-11\n\nLet's be clear. That is the equlibrium constant for the reaction whereby the hydrogen carbonate loses a proton:\n\nHCO3- --> H+ + CO3-2
434401
I am pretty sure i did this right. using the CaCO3(s)as the limestone, i got 1178.934669 grams of CaO. (I didn't round the final answer, and w/in the problem itself, i rounded the atomic masses of Calcium (to 40.1), oxygen (to 15.9), and carbon (to 12)
99720
Atomic mass is based on the average amu (atomic mass units) of C 12 therefore 35.5 amu is the average atomic weight for Cl 17
808850
Great problem!  OK, weigh the chalk before and after you write your name.  Assuming no chalk dust, then the difference in weight is the amount that it took.  Let's say that the amount is 1.0009.  The molecular weight of calcium carbonate is 100.09, so you've used (1.0009/100.09) = 0.01 moles of CaCO3.  Using Avogadro's number, this would be 0.01 moles x 6.023 x 10^23 molecules/mole or 6.023 x 10^21 molecules.  So you have that many calcium atoms, that many carbon atoms, and three times that many oxygen atoms.
287378
Mass spectrometers are only able to record the total weight on an atom that passes through. Since oxygen isotopes are measured by reacting calcium carbonate with acid to form carbon dioxide, the mass spectrometer reveals the molecular weight of each carbon dioxide molecule. Assuming carbon-12, there are then 6 possible combinations of carbon dioxide that the mass spectrometer will record.\n\nThe oxygen combinations can be O-16 and O-18; O-16 and O-17; O-16 and O-16; O-17 and O-17, O-17 and O-18, and O-18 and O-18. The mass spectrometer will then record masses of 46, 45, 44, 46, 47, and 48 for these. So you can see that you will not be able to tell the difference between O-16/O-18 and O-17/O-17 because they both come to 46. That is why you have to independently determine how much O-17 is in the sample and correct for the ambiguity.
308860
The molecular weight of acetaldehyde is 44.053 amu.  A good site to go to for questions about simple organic molecules is http://www.chemfinder.com.\n\nThe person below me used only whole numbers for the masses of the atoms.  Carbon doesn't weight 12 amu, it weighs 12.011 amu and Hydrogen weighs 1.008 amu.
95148
Actually, the mass of a proton is 1.00727664669 atomic mass units.\n\nAn atomic mass unit is defined such that Carbon 12 is exactly 12.  The carbon atom weighs less than 12 times the proton (because of nuclear binding energy).
778176
Use the periodic table of the elements.  The "weights" are in grams per mol.  Just use algebra and solve for the number of mols.  Then you know how many atoms there are by the number of mols which is a definite number.
844511
Carbon Dioxide means "Carbon and two (di) oxygens".  Which means it's CO2\n\nMost of the other ones you asked can be figured out the same way.\n\n"Mon" = 1\n"Di" = 2\n"Tri" = 3\n"Tetra" = 4\n\nYou're not doing yourself any favors by having everyone else tell you all the answers - you need to LEARN this stuff, not just copy and paste someone else's answers.
41822
Simple one will be \nSunlight + Carbon dioxide (CO2) + Water (H2O)--> Glucose (C6H12O6) + Oxygen (O2).\nor \n6CO2 +12 H2O (light energy and chlorophyll) ---> C6H12O6 + 6O2\nRemember to use subscript whenever necessary.
912145
CO2 - the carbon atoms possibly are derived from hydrocarbons in food, and the oxygen atoms are, of course, from the atmosphere.
882871
From the ideal gas law, we can get the number of moles (n):\nPV=nRT\nT = 50.8°C = 323.95 K\n.980 atm * 1.00 L = n * 8.2057 E-2 L*atm / (mol*K) * 323.95 K\nn = 0.03687 mol\nSo, the molecular weight, MW = m/n = 2.58 g / .03687 mol = 69.98 g/mol\n\nThe mass % of C is 85.62%, so the mass% of H has to be 14.38%\n\nIt you had 1 mole of the gas, it would weigh 69.98 g\n\n69.98 g * 85.62% = 59.92 g\n69.98 g * 14.38% = 10.06 g\n\nThe atomic weight for carbon is about 12:\n59.92g / 12 g/mol = 4.99 mol = 5 mol\n\nThe atomic weight of hydrogen is about 1:\n10.06g / 1 g/mol = 10.06 mol = 10 mol\n\nSo, your molecular fomula is C5H10\n\nThis can be several different forms:\n\nCH3-CH=CH-CH2-CH3, 2-pentene\nCH2=CH-CH2-CH2-CH3, 1-pentene\nC5H10, Cyclopentane\nCH3-CH(CH3)-CH=CH2, 2-methyl-1-butene\nThe list goes on...
762399
I really don't know and as much as i don't know, i hope this helps.\n\nhttp://physics.nist.gov/PhysRefData/CO2/Html/chap1.html
428107
first count molecules of carbon in CH3Co2H, in this case its one, 12.01 grams of carbon in each mole of CH3Co2H, divide 12.01 by the total weight mass of CH3Co2H which is 133.91 and you get .0897 or 8.97%
205870
CaCO3(s) + 2HC2H3O2(aq)-> Ca(C2H3O2)2(aq) + H2O(l) + CO2(g)
799022
I'm assuming you really mean "How do you find out how many atoms of a element are in a particular compound?"\n\nJust multiply the subscript by the coefficient\n\nEx. 2 molecules of carbon dioxide. The coefficient is 2 and the subscript for carbon is 1. Therefore there are 2*1=2 atoms of carbon in 2 molecules of carbon dioxide.\n\nIf you just want the amount in one molecule, just substitute 1 for any coefficient you have.\n\nIf you cannot see any subscripts and/or coefficients for the element you are looking at, the subscript and/or coefficient is 1.