Molecular Formulas 1.Find empirical formula 2.Calculate molar mass of empirical formula 3.Molar mass...
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Transcript of Molecular Formulas 1.Find empirical formula 2.Calculate molar mass of empirical formula 3.Molar mass...
![Page 1: Molecular Formulas 1.Find empirical formula 2.Calculate molar mass of empirical formula 3.Molar mass of compound / molar mass of empirical formula (we’ll.](https://reader036.fdocuments.us/reader036/viewer/2022082610/56649da15503460f94a8da47/html5/thumbnails/1.jpg)
Molecular Formulas
1. Find empirical formula
2. Calculate molar mass of empirical formula
3. Molar mass of compound / molar mass of empirical formula (we’ll call this the factor)
4. Multiply subscripts by factor to get molecular formula
![Page 2: Molecular Formulas 1.Find empirical formula 2.Calculate molar mass of empirical formula 3.Molar mass of compound / molar mass of empirical formula (we’ll.](https://reader036.fdocuments.us/reader036/viewer/2022082610/56649da15503460f94a8da47/html5/thumbnails/2.jpg)
Molecular Formula• A compound is found to have an empirical formula of
C2H3O2. The molar mass of the compound has 118.1 g/mol. What is the molecular formula?– Molar mass of C2H3O2
C2H3O2 = 2x12 + 3x1 + 2x16= 59 g/mol
– Molar mass of compound / molar mass of empirical118.1 / 59 = 2
464
xxx
232
222
OHC
OHC
![Page 3: Molecular Formulas 1.Find empirical formula 2.Calculate molar mass of empirical formula 3.Molar mass of compound / molar mass of empirical formula (we’ll.](https://reader036.fdocuments.us/reader036/viewer/2022082610/56649da15503460f94a8da47/html5/thumbnails/3.jpg)
Molecular Formula• A compound was found to contain 49.98 g
carbon and 10.47 g of hydrogen. The molar mass of the compound is 58.12g/mol. Determine the molecular formula
• C= 49.98 / 12 = 4.165 / 4.165 = 1 x 2 = 2• H= 10.47 / 1 = 10.47 / 4.165 = 2.5 x 2 = 5
• C2H5 = 2x12 + 5x1 = 29• 58.12 /29 = 2
C2H5x2 x2
C4H10
![Page 4: Molecular Formulas 1.Find empirical formula 2.Calculate molar mass of empirical formula 3.Molar mass of compound / molar mass of empirical formula (we’ll.](https://reader036.fdocuments.us/reader036/viewer/2022082610/56649da15503460f94a8da47/html5/thumbnails/4.jpg)
Molecular Formula Practice I1. Analysis of a chemical used in photographic
developing fluid indicates a chemical composition of 65.45% C, 5.45% H, and 29.09% O. The molar mass is found to be 110 g/mol. Determine the molecular formula.
![Page 5: Molecular Formulas 1.Find empirical formula 2.Calculate molar mass of empirical formula 3.Molar mass of compound / molar mass of empirical formula (we’ll.](https://reader036.fdocuments.us/reader036/viewer/2022082610/56649da15503460f94a8da47/html5/thumbnails/5.jpg)
Molecular Formula Practice I2. A compound was found to contain 49.98 g carbon
and 10.47 g hydrogen. The molar mass of the compound is 58.12 g/mol. Determine the molecular formula.
![Page 6: Molecular Formulas 1.Find empirical formula 2.Calculate molar mass of empirical formula 3.Molar mass of compound / molar mass of empirical formula (we’ll.](https://reader036.fdocuments.us/reader036/viewer/2022082610/56649da15503460f94a8da47/html5/thumbnails/6.jpg)
Molecular Formula Practice I3. A colorless liquid composed of 46.68% nitrogen
and 53.32% oxygen has a molar mass of 60.01 g/mol. What is the molecular formula?