Grams/moles
The molar mass is expressed in grams.
molacular mass
This is equal to the molar mass of this substance.
The molar mass is 228,1 g.
molar mass of unknown/molar mass of empirial = # of empirical units in the molecular formula. Example: empirical formula is CH2O with a molar mass of 30. If the molar mass of the unknown is 180, then 180/30 = 6 and molecular formula will be C6H12O6
The molar mass is expressed in grams.
molacular mass
The molar mass is the mass of a molecule - sum of the masses of contained atoms, expressed in grams.The atomic mass is the mass of an isotope expressed in unified mass atomic units.The atomic weight is the mass of a chemical element (taking into account its isotopes) expressed in unified mass atomic units; also known today as relative atomic mass. IUPAC maintain the term (standard) atomic weight.
g/mol
This is equal to the molar mass of this substance.
Average weight of an element expressed in Atomic Mass units.
Mass is not expressed in kilometers (km). That is a measure of distance. Mass is expressed in units of kilograms (kg)
The molar mass of a compound is expressed in grams.
molar mass is the actual mass of the one atom but relative mass is the average isotopes of the atoms.------------------------------------------Atomic mass is the mass of an isotope, expressed in atomic mass units.Molar mass is the mass of molecule, calculated from the atomic weights of the contained chemical atoms, expressed in grams.
The molar mass is 228,1 g.
The formulaic conversion between atomic mass units and SI mass in grams for a single atom is:where Mu is the Molar mass constant and NA is Avogadro's number.The number of atoms in a mole is calledAvogadro's number, the value of which is approximately 6.022 × 1023 mol-1One mole of a substance always contains almost exactly therelative atomic mass or molar mass of that substance (which is the concept of molar mass), expressed in grams ..>> that's all thank you!! :)) ~ ^^
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.