To convert mass to atoms: Find the atomic mass of the element in the substance. You can find atomic masses on the periodic table.

The units in which the mass of an atom are expressed are atomic mass units. Program Do Lamania Hasla Na Facebooku Chomikuj Filmy. At one time, the lightest atom was assigned a mass of 1 amu and the. By definition, aa mole of any substance contains the same number of elementary particles as there are atoms in exactly 12 grams of the 12C isotope of carbon. How do you convert molecules to grams? Update Cancel. Fill those values of g (mass in grams). How do you convert grams to atoms?

Lithium's atomic mass is 6.9 grams (round if you need to) Then find the mass of the substance in grams. You have 18.2 grams of a sample of Lithium. The mass of the sample is multiplied by 6.02 * 1023 and divided by the atomic mass. Mass of sample in grams * (6.02 * 1023 atoms) / (atomic mass) = # atoms in grams 18.2 grams * (6.02 * 1023 atoms) / (6.9 grams) = 1.59 * 10 24 atoms The number 6.02 * 1023 is Avogadro's Constant which is the amount of atoms (or molecules) in one mole. To convert mass to atoms: Find the atomic mass of the element in the substance.

You can find atomic masses on the periodic table. Lithium's atomic mass is 6.9 grams (round if you need to) Then find the mass of the substance in grams. You have 18.2 grams of a sample of Lithium. The mass of the sample is multiplied by 6.02 * 1023 and divided by the atomic mass. Mass of sample in grams * (6.02 * 1023 atoms) / (atomic mass) = # atoms in grams 18.2 grams * (6.02 * 1023 atoms) / (6.9 grams) = 1.59 * 1024 atoms The number 6.02 * 1023 is Avogadro's Constant which is the amount of atoms (or molecules) in one mole. Moles to atoms you multiply the number of moles by avogadros number ex: 1.32 mol x (6.022 x 10^23 atoms)/mol mass to atoms you multiply the mass (in grams) times the molar mass of the element or compound (ex: N 14.01 mols/gram) then times avogadros number once you have the moles. Ex: 45.6 g N x (14.01 mol/gram) x (6.022 x 10 ^23 atoms/mol) if it's a compound instead of an element, find the molar mass of the compound (the molar masses of all the elements in it added up) and multiply by it.

------------------------- Actually you are wrong, from mass to atoms you need to take the initial mass divide by the gram of the element that you are doing and multiply by the Avogadros number.

Express the relationship of the three pieces of information you need to calculate the number of atoms in the sample in the form of an equation. Scientists express atomic weights in terms of grams per mole, so the resulting equation looks like this: atomic weight expressed in atomic mass units = grams/mole. In scientific notation, it would appear like this: u = g/mole. Look up the sample's atomic weight on a periodic table of the elements. For example, boron has an atomic weight of 10.811 atomic mass units which you could also express as 10.811 grams per mole of the element. Plugging that figure into the above equation would look like this: 10.811 = g/mole.

Solve the equation for the unknown quantity; if u = g/mole and you have a number for u and g, then the number of moles is your target. Multiply everything through by the divisor to isolate the unknown quantity and you will reach an equation that looks like this: mole = g/u, where g equals the sample's weight in grams and u equals the element's atomic weight in atomic mass units.

Divide the grams of your sample by its atomic weight to derive the number of moles the sample contains. If your sample of boron weighed 54.05 g, your equation would look like this: mole = 54.05/10.811. In this example, you would have 5 moles of boron. Multiply the number of moles in the sample by Avogadro's number, 6.02 x 10^23, to derive the number of atoms in the sample. In the given example, multiply Avogadro's constant by 5 to discover that the sample contains 3.01 x 10^24 individual boron atoms. Check your work to ensure that it makes sense.

Negative numbers, small numbers and numbers that do not seem to fit with the sample size mean a mathematical error.