How many atoms are in a mole?
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I will now quote part of a song our chemistry teacher taught us by Michael Offut\n\n"A mole is a unit, or have you heard?\n Containing 6.02 times 10 to the twenty-third" \n\nor 6.02*10^23
930413
6.37 moles of any molecular substance just contains 6.37 times Avogadro's number of molecules, because a mole of matter always contains a mole of particles, that is, Avogadro's number many.  6.37*6.022 x 10^23 = 3.84 x 10^24.
561143
23.5 X the molcular weight of what ever it is X Avogadro's number (6.0221415 × 10^23 ) = the number of atoms or molecules in 23.5 grams.
136398
Avagodro's number\n\nAvogadro's number and the mole are very important to the understanding of atomic structure. The Mole is like a dozen. You can have a dozen guitars, a dozen roosters, or a dozen rocks. If you have 12 of anything then you would have what we call a dozen. The concept of the mole is just like the concept of a dozen. You can have a mole of anything. The number associated with a mole is Avogadro's number. Avogadro's number is 602,000,000,000,000,000,000,000 (6.02 x 1023). A mole of marbles would spread over the surface of the earth, and produce a layer about 50 miles thick. A mole of sand, spread over the United States, would produce a layer 3 inches deep. A mole of dollars could not be spent at the rate of a billion dollars a day over a trillion years. This shows you just how big a mole is. This number is so large that it is usually only represented in scientific notation.\n\nProbably the only thing you will ever have a mole of is atoms or molecules. One mole of magnesium atoms (6.02 x 1023 magnesium atoms) weigh 24.3 grams. 6.02 x 1023 carbon atoms weigh a total of 12.0 grams. 6.02 x 1023 molecules of CO2 gas only weigh a total of 44.0 grams. The decimal number on the periodic table is the atomic mass, the mass of one atom measured in atomic mass units(amu). Amu's are defined to be 1/12 the weight of the most common isotope of Carbon. This number in grams is the mass of 1 mole of that element. For example, 6.02 x 1023 iron atoms weigh only 55.847 grams.(This is equivalent to saying one mole of iron atoms weighs 55.847 grams.) One mole of sulfur weighs 32.066 grams. (This is the same as saying 6.02 x 1023 Sulfur atoms weigh 32.066 grams)\n\nWhen not measured in grams, the decimal number on the periodic table is called the atomic mass and is in atomic mass units(amu). As mentioned earlier, one proton weighs 1.0073 amu and 1 neutron weighs 1.0087 amu. So the atomic mass is the mass in amus of one atom of an element, but you rarely use the mass of one atom. Even if you have a tiny speck of a metal or a microgram of an element, you have billions and billions of atoms. Thus, the mass in grams of one mole of an element (the gram atomic weight) is more useful.
973794
moles = concentration* volume\n\nfind the moles of the substance with given concentration and volume\n\n\nwrite and balance the equation. determine the moles equivalence of every reactant then use the equation above
541177
A mole is 6.23 x 10^23 of something.  That number is Avogadro's number.  So a mole of Helium atoms is 6.23 x 10^23.  The weight listed on the periodic table is also the weight of a mole of atoms of a pure element in grams.\n\nThey are used because it gives us a nice round number to work with.  Some reactions require 2 of one molecule and 3 of another for example.  Well, 2 molecules and 3 molecules are hard to work with.  So instead, we could use 2 and 3 moles of the compounds and do the reaction, without having to worry about the molecular weights as much or densities or other physical properties.  Hope that makes sense.
34174
(X atoms)/(6.02x10^23 atoms/mol) = Y moles\n\n(Y moles)*(6.02x10^23 atoms/mol) = X atoms
179528
1 mole of a substance means 6.023 x 10^23 molecules..so thr will be 6.023 x 10^23 no of carbon disulphide molecules. now each CS2 molecule has one carbon and 2 sulphur atoms  .so there will be 6.023 x 10^23 atoms of carbon and 2 x 6.023 x 10^23 sulphur atoms
447953
Copper's atomic mass is 63.55 grams/mole.  There are 6.02*10^23 copper atoms in mole of copper.  Thus, 1 atom Cu * 1 mol Cu/6.02*10^23 atoms Cu * 63.55 gCu/1 mol Cu = 1.056 * 10^-22 grams/atom Cu
211095
One mole of iodine weighs 126.90447grams/mole.\n\nIf you are looking for any more information about iodine please check the webelements link below.
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1 mole of anything has 6.02x10^23 items...kinda like 1 dozen of anything has 12 items in it\n\nso....1 mole of Li would have  6.20x10^23  atoms\n\n3.66 moles of LIthim x 6.20x10^23 = 2.205 X 10^24 atoms
769656
An atom is the smallest particle of matter.\n\nA mole is quantity of something.  A mole of something (anything) is 6.02 x 10^23.  Whether it's buses, frogs, statues, whatever.  It is however often used to describe a quantity of atoms or molecules.
1097097
For grams to mole, you find the molar mass of whatever substance you're working with (add the atomic masses together--it's the number with the decimal on the periodic table), and then put the number of grams you have of the substance over the molar mass.  That gives you the number of moles in the substance.\n\nFor moles to molecules, there are exactly 6.022 x 10^23 molecules of a substance per mole.  That's Avogadro's number.  Simply multiply the number of moles times Avogadro's number and you have the number of molecules.\n\nFor moles to ideal gases, there are 22.4 liters of an ideal gas at standard temperature and pressure per mole of gas.  Multiply your number of moles by 22.4 and you'll have how many liters.
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Molecules are made of atoms
700696
First you change grams to moles:\n2.3 x 10^-4 grams Si  |  1 mole Si\nbig open space here  |   28.09 g Si\n\n= 8.19 x 10^-6 moles\n\nThen you change moles to molecules:\n8.19 x 10^-6 moles   |  6.02 x 10^23 molecules\nbig open space here|   1 mole\n\n= 4.93 x 10^18 molecules Si\n\nYou always multiply what's on top and divide by what's on the bottom.
961946
one mole of a substance is 6.02x10^23 (avogadro's number) atoms. so... you have one mole.\nso from this, there would be 22.99 grams.\n\nexplained:\nn(moles) = m(mass) / M(molecular wt.)\n1 = m / 22.99\nm = 1 * 22.99\nm = 22.99 g \n\n:-)
851404
At room temperature and pressure one mole (6 x 10^23 particles/atoms/molecules) of a gas fills 24 dm^3 (Litres).\n\nThis means that in every cubic centimeter (one millilitre) of air there are 2.5 x 10^19 molecules.\n\nIf we forget about the rapid movement and think how many static molecules this means in each dimension we find that each 1-dimensional 1-cm long line contains 2,924,017 molecules (let's say 3 million to keep things simpler).\n\nOver 70% of air is Nitrogen and the length of an N2 molecule is about (keeping things simple) 100 pm (picometers; 10^-12 m) so 3 million molecules take up 300 million picometers or 300 micrometers (following conversion)\n\nThere are 10,000 micrometers in a centimeter so the molecules only 3% of the available distance.\n\nIf all 3 million molecules were equally spaced they would be approximately 3.3 nm (nanometers; 10^-9 m) apart.\n\nA division of the molecular length (100 pm) by the separation (3.3 nm) shows that they are about 33 molecules length apart.\n\nNow I've made plenty of assumptions here. I'm more than happy for people to point out where I've gone wrong (if I have). Please PM me.