a mass of 6.005grams of carbon with an atomic mass of 12.010atomic mass contains?
823661
Using the numbers given, it contains a half a mole of carbon.  Note that the atomic mass of carbon given pertains to a natural mixture of isotopes C12 and C13; the atomic mass of C12 is 12.00000 by definition.
730167
Very close to the mass of a proton.  It is about 1.6749 x 10^-27 kg, 1 u, or 939.57 MeV/c^2.
969783
1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 6.406 g x (12 / 44) = 1.747 g\nhydrogen: 5.244 g x (2 / 18) = 0.583 g\noxygen: 4.664 - 1.747 - .583 = 2.334 g\n\n2) convert to moles.\ncarbon: 1.747 / 12 = 0.146 mol\nhydrogen: 0.583 / 1 = 0.583 mol\noxygen: 2.334 / 16 = 0.146 mol\n\n3) divide each molar amount by the lowest value\ncarbon: 0.146 / 0.146 = 1\nhydrogen: 0.583 / 0.146 = 4\noxygen: 0.146 / 0.146 = 1\n\nWe have now arrived at the answer: the empirical formula of the substance is CH4O.\nThe atomic masses add up to 32, which is also the molar mass of the compound.
89857
C6H12O6 represents Glucose and Fructose. Go to http://images.google.com/images?q=Glucose%20structure
812589
You must remember the center of mass equation:\n\n(m[1]x[1] + m[2]x[2])/(m[1] + m[2]).\n\nm[1] can be called mass of carbon atom - 12\nm[2] can be called mass of oxygen atom- 16\n\nArbitrarily pick the carbon atom as the origin thus x[1]- 0m\nThe oxygen atom is 1.13 X 10^-10m away from the carbon atom (origin)- x[2]- 1.13 X 10^-10m.\n\nThe answer you will get is 6.5 X 10^-11. This is the distance of the center of mass RELATIVE to the origin, since the origin is the carbon atom, the carbon atom is located 6.5 x 10^-11m away from the center of mass.\n\nHope that helps, I tried to be thorough.
87474
750 milliamps. (P=IxE)
791445
It's composed of the most common isotope of carbon and hydrogen which is carbon-12 and hydrogen-1.\n\nCarbon-12 has 6 protons, 6 neutrons and 6 electrons.\n\nHydrogen-1 has 1 proton and 1 neutron.\n\nSo...\n\nProtons: (6 + 1) * 6 = 42\nNeutrons 6 * 6 = 36\nElectrons (6 + 1) * 6 = 42
751778
1 mole of an element= 6.022x10^23 atoms\n1 mole of an element weighs the molecular weight of the element in grams
131302
it has a relative molecular mass of 40 g/mole
759497
1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 7.432 g x (12 / 44) = 2.027 g\nhydrogen: 4.057 g x (2 / 18) = 0.451 g\noxygen: 3.383 - 2.027 - .451 = 0.905 g\n\n2) convert to moles.\ncarbon: 2.027 / 12 = 0.169 mol\nhydrogen: 0.451 / 1 = 0.451 mol\noxygen: 0.905 / 16 = 0.0566 mol\n\n3) divide each molar amount by the lowest value to obtain small integers\ncarbon: 0.169 / 0.0566 = 3\nhydrogen: 0.451  / 0.0566 = 8\noxygen: 0.0566 / 0.0566 = 1\n\nThe empirical formula of the substance is (C3H8O)n\nThe atomic masses add up to 60, which is also the molar mass of the compound. Therefore n=1 and we find C3H8O
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).
995643
Becasue if you take the constituent atoms of a carbohydrate molecule and break them down, you could put them together to form water and carbon.\n\nFor example, sucrose -- C12H22O11 -- could be broken down into 12 atoms of carbon and 11 molecules of water.
413959
Well, this is a simple factor labelling problem... I hope you aren't using this to have people do your homework... ;)\n\n1pound x (454 grams/pound) x (1 mol H atoms/1.0079g H atoms) x (6.022x10^23 H atoms/1 mol H atoms) = 2.71 x 10^26 H atoms\n\nnote to PaulB_23: periodic tables are in amu, which is also a ratio of grams per mole, not moles per kg, the 1.008 would just be 1.0079 rounded, I just went w/ a slightly more accurate #
384517
(12/12+16)*100=42.85\n12---------atomic mass of carbon\n16---------atomic mass of oxygen
745918
The Mole was not so much "discovered", but arbitrarily created. (Much like any other unit of measure). All this means is that scientists agreed upon a specific amount that will represent 1 mol of a substance. This amount was related to every element based on its average atomic mass value, which in the case of moles is named the molar mass. Each element has a different molar mass, which is why 12g of carbon is one mole, whereas 12g of oxygen is only 0.75 moles.\nOne mole represents a value of 6.022x10^23 atoms of elements, or 6.022x10^23 molecules of a substance. This number is Avogadro's number, and is the "number" behind a mole.\nAs this is an SI unit (Système Internationale) I believe this concept was first introduced by French Scientists.
914156
6 CO2 + 12 NADPH + 12 H+ + 18 ATP → C6H12O6 + 6 H2O + 12 NADP+ + 18 ADP + 18 Pi
702947
The atomic weight is the mass in grams per mole (atomic mass of iron = 55.845).\n\nA mole is 6.02 x 10^23 atoms, therefore the mass of 500 atoms would be:\n\n500/(6.02x10^23) x 55.845 = 4.64 x 10^-20 grams.\n\nNotice that's 10 to the -20 power.