Ca = 40 x 3 = 120 grams
P = 31 x 2 = 62 grams
O = 16 x 8 = 128 grams
Add them together and you have 310 grams. This is the mass in grams of your formula. It is expressed in grams/mole because 310 is the weight of one mole of
Ca3(PO4)2.
The gram-formula mass of a compound is the sum of the atomic masses of all the atoms in a formula unit of the compound. For NO2, the gram-formula mass is calculated by adding the atomic mass of nitrogen (N) and two times the atomic mass of oxygen (O).
Nitrogen hydride has the chemical formula of NH3 The gram formula mass of nitrogen is approximately 14.0 g/mole & the gram formula mass of hydrogen is approximately 1.0 g/mole In the chemical formula, you have 1 nitrogen atom and 3 hydrogen atoms 14.0 + 1.0 + 1.0 + 1.0 = 17.0 g/mole
The grand formula mass is the sum of the masses of all the atoms in a single molecule of a compound, including all elements present in that compound. It is calculated by adding up the atomic masses of each element involved in the molecule.
The empirical formula of SN has a formula unit mass of the sum of the gram atomic masses of nitrogen and sulfur, i.e., about 46.0667. The gram molecular mass given in the problem divided by this formula unit mass is about 4. Therefore, the molecular formula is S4N4.
The gram formula unit mass of sodium chloride is 58.443, and every gram formula unit mass contains Avogadro's Number, 6.022 X 1023 formula units. Therefore, the mass sought is 58.443 X (4.59 X 1024)/(6.022 X 1023) or 445 grams, to the justified number of significant digits.
The gram formula for potassium sulfite (K2SO3) is 158.27 g/mol.
The formula of sodium fluoride is NaF; its gram formula mass is 41.9882.
H2O's molar mass is 18 g/mol.
The gram formula mass of sodium (Na) is approximately 23 grams per mole.
The mass of a mole of an ionic compound.
The gram formula mass of acetic acid (CH3COOH) is approximately 60.05 g/mol.
To determine the molecular formula from the empirical formula and gram formula mass, first calculate the empirical formula mass of C4H9 (4 carbons + 9 hydrogens). Then, divide the gram formula mass by the empirical formula mass to find the ratio. Finally, multiply the subscripts in the empirical formula by this ratio to get the molecular formula, which in this case is C8H18.
The gram-formula mass of a compound is the sum of the atomic masses of all the atoms in a formula unit of the compound. For NO2, the gram-formula mass is calculated by adding the atomic mass of nitrogen (N) and two times the atomic mass of oxygen (O).
when atomic mass of an element expressed in gram atom is called gram atom mass . and formula is number of gram atom=given mass (in gram) by atomic mass ( in gram )
The atomic mass number of nitrogen is 14.0
From the Periodic Table The Atomic mass of Nitrogen (N) is 14 The Atomic mass of Oxygen (O) is 16 Hence the gram formula mass of NO is 14 + 16 = 30 Now NO under certain circumstances can form N2O2 hence the gram formula mass of N2O2 = (2 x 14) + ( 2 x 16) = 28 + 32 = 60 However the empirical formula is the formula with the lowest ratio of atoms. Hence N2O2 lowest ration is NO # formula mass is 30 .
The gram molecular mass of the molecule must be measured by some independent method such as freezing point depression or boiling point elevation. Then the factor by which to multiply all of the subscripts in the empirical formula to get the molecular formula is the closest integer to the ratio of gram molecular mass to the gram molecular mass of a single unit of the empirical formula.