Wiki User
∙ 13y agoThere is no direct relationship between atoms of boronand grams of boron. Use Avogadro's number to convert atoms to moles, and the atomic mass to convert moles to grams.
Since you are converting from atoms B, this goes in the denominator (on the bottom) of the first factor. You want to end up in units of grams of B, so this goes in the numerator (on the top) of the last factor.
atoms B1.00 mole B10.8 gram = g B6.02E+23 atom B1.00 mole B
Note that the units atoms boron "cancel out" in the first factor and you are left in units of moles. Moles cancel outin the second factor and the final units are grams boron.
Wiki User
∙ 13y agoTo convert atoms of boron to grams of boron, you would multiply by the molar mass of boron, which is approximately 10.81 grams per mole. This conversion allows you to relate the number of atoms to the mass in grams.
You would multiply the number of atoms of germanium by its atomic mass, which is approximately 72.6 grams/mol, to convert atoms to grams. This conversion allows you to determine the mass of germanium in grams.
The mass of a boron atom is approximately 10.81 atomic mass units (amu). In grams, this would be about 1.80 x 10^-22 grams.
To calculate the mass of the atoms of nickel, you need to multiply the number of atoms by the atomic mass of nickel. The atomic mass of nickel is approximately 58.6934 g/mol. Therefore, the mass of 9.3 x 10^15 atoms of nickel would be approximately 3.48 x 10^-8 grams.
The atomic weight of boron is approximately 10.81 atomic mass units.
To find the number of moles in 97.2 grams of boron, you need to divide the mass given by the molar mass of boron. The molar mass of boron is approximately 10.81 g/mol. Therefore, 97.2 grams of boron is equal to 97.2/10.81 ≈ 8.98 moles.
You would multiply the number of atoms of germanium by its atomic mass, which is approximately 72.6 grams/mol, to convert atoms to grams. This conversion allows you to determine the mass of germanium in grams.
To convert grams of oxygen to atoms of oxygen, you would multiply by Avogadro's number, which is approximately 6.022 x 10^23 atoms/mol. This conversion allows you to move from the unit of mass (grams) to the unit of atoms.
The mass of a boron atom is approximately 10.81 atomic mass units (amu). In grams, this would be about 1.80 x 10^-22 grams.
10.81g This is found by looking at the atomic weight. The atomic weight refers to the mass of a singe atom in units of AMU (atomic mass units) and it also refers to the mass of one mole of the element in grams.
The mass is 2.86 grams but the weight will be 0.028 Newtons.
A conversion is the change between two units (usually units of measurement). For example... if you have 2 kg and you want to find out how many grams are in it, you multiply by the amount of grams there are in ONE kilogram, 1000. Therefore, 2 times 1000 is 2000 grams.
FORMULA UNITS TO MOLES (formula units --> moles)Divide the number of formula units by Avogadro's number.----------- Formula UnitsAvogadro's number (formula units)Conversion FactorFormula Units x 1 mol-------- Avogadro's number (formula units)MOLES TO FORMULA UNITS (moles --> formula units)Multiply the number of moles by Avogadro's number.Moles Substance x Avogadro's numberConversion FactorMol substance x Avogadro's number---------------------- 1 mol substanceMOLES TO GRAMS (moles --> grams)*Multiply the number of moles by the substance's molar mass.Moles Substance x Molar Mass SubstanceConversion FactorMol Substance x Molar Mass Substance------------------------- 1 mol SubstanceGRAMS TO MOLES (grams --> moles)*Divide the number of grams by the substance's molar mass.---- Mass (g) SubstanceMolar Mass (g) SubstanceConversion FactorMass (g) Substance x 1 mol substance----------------------- Molar Mass Substance (g)FORMULA UNITS TO GRAMS (formula units --> moles --> grams)*Divide formula units by Avogadro's number (6.022 x 1023 formula units); multiply by molar mass.--- Formula Units --- x --- Molar MassAvogadro's numberConversion FactorFormula Units x 1 mol ----------------- x -------------- Molar mass (g)---------- Avogadro's number (formula units) ----------- 1 molGRAMS TO FORMULA UNITS (grams --> moles --> formula units)*Divide mass of substance by the molar mass of substance; multiply by Avogadro's number.---- Mass (g) substance -- x -- 6.022 x 1023 moleculesMolar mass (g) substanceConversion Factor--- Mass substance (g) x 1 mol substance ------ x ----- Avogadro's number------------------------ Molar Mass (g) substance ----------- 1 mol substanceTip: On test day, anytime you see the words ions, formula units, molecules, or atoms on a question, that problem will involve the usage of Avogadro's number.*Finding Molar Mass# Atoms Element A x Atomic Mass Element A (Periodic Table) = mass (g) El. A# Atoms Element B x Atomic Mass Element B (Periodic Table) = mass (g) El. B... etc.Add up all the mass values found above and you have molar mass.
This can be found using one of the most important constants for chemistry: Avogadro's number. According to wikipedia, the standard atomic weight of magnesium is 24.3050 grams per mole. Using Avogadro's number, we know there's 6.0221415 × 1023 atoms per mole, so if you divide the standard atomic weight of magnesium by Avogadro's number, you can get number of grams per atom of magnesium (i.e. the mass of a single magnesium atom in grams). (24.3050 g/mole) / (6.0221415 x 1023 atoms/mole) = 4.03564 g/atom
grams of mercury (Hg) 1 mole x 1 mole Avogadro's number (6.022 x 1023) of atoms 200.6 grams Hg 1 mole 200.6 grams Hg = x = ≈ 3.3311192-23 atoms Hg 1 mole 6.022 x 1023 atoms 6.022 x 1023 atoms
Atomic Mass Number Of Boron.The Atomic Mass Number Of Boron Is 10.81 Its Atomic number is 5. It has 5 p neutrons , 6 neutrons and 5 electrons. Its valency is 3. it has 3 valence electrons.
To convert grams to atomic mass units (amu), you need to divide the grams by the molar mass constant, which is 1 gram/mol. In this case, 1.18 grams would be equivalent to 1.18 amu.
The unit of weight for elements is typically measured in atomic mass units (amu) or grams. The atomic mass unit is defined as one twelfth of the mass of a carbon-12 atom.