How many grams Antimony Dichlorotrifluoride in 1 mol?
The answer is 249.6612096.
We assume you are converting between grams Antimony Dichlorotrifluoride and mole.
You can view more details on each measurement unit:
molecular weight of Antimony Dichlorotrifluoride or mol
The molecular formula for Antimony Dichlorotrifluoride is SbCl2F3.
The SI base unit for amount of substance is the mole.
1 grams Antimony Dichlorotrifluoride is equal to 0.0040054280022202 mole.
Note that rounding errors may occur, so always check the results.
Use this page to learn how to convert between grams Antimony Dichlorotrifluoride and mole.
Type in your own numbers in the form to convert the units!
1 grams Antimony Dichlorotrifluoride to mol = 0.00401 mol
10 grams Antimony Dichlorotrifluoride to mol = 0.04005 mol
50 grams Antimony Dichlorotrifluoride to mol = 0.20027 mol
100 grams Antimony Dichlorotrifluoride to mol = 0.40054 mol
200 grams Antimony Dichlorotrifluoride to mol = 0.80109 mol
500 grams Antimony Dichlorotrifluoride to mol = 2.00271 mol
1000 grams Antimony Dichlorotrifluoride to mol = 4.00543 mol
You can do the reverse unit conversion from moles Antimony Dichlorotrifluoride to grams, or enter other units to convert below:
grams Antimony Dichlorotrifluoride to kilomol
grams Antimony Dichlorotrifluoride to millimol
grams Antimony Dichlorotrifluoride to micromol
grams Antimony Dichlorotrifluoride to picomol
grams Antimony Dichlorotrifluoride to nanomol
grams Antimony Dichlorotrifluoride to molecule
grams Antimony Dichlorotrifluoride to centimol
grams Antimony Dichlorotrifluoride to atom
grams Antimony Dichlorotrifluoride to decimol
In chemistry, the formula weight is a quantity computed by multiplying the atomic weight (in atomic mass units) of each element in a chemical formula by the number of atoms of that element present in the formula, then adding all of these products together.
Using the chemical formula of the compound and the periodic table of elements, we can add up the atomic weights and calculate molecular weight of the substance.
The atomic weights used on this site come from NIST, the National Institute of Standards and Technology. We use the most common isotopes. This is how to calculate molar mass (average molecular weight), which is based on isotropically weighted averages. This is not the same as molecular mass, which is the mass of a single molecule of well-defined isotopes. For bulk stoichiometric calculations, we are usually determining molar mass, which may also be called standard atomic weight or average atomic mass.
A common request on this site is to convert grams to moles. To complete this calculation, you have to know what substance you are trying to convert. The reason is that the molar mass of the substance affects the conversion. This site explains how to find molar mass.
Formula weights are especially useful in determining the relative weights of reagents and products in a chemical reaction. These relative weights computed from the chemical equation are sometimes called equation weights.
If the formula used in calculating molar mass is the molecular formula, the formula weight computed is the molecular weight. The percentage by weight of any atom or group of atoms in a compound can be computed by dividing the total weight of the atom (or group of atoms) in the formula by the formula weight and multiplying by 100.
Finding molar mass starts with units of grams per mole (g/mol). When calculating molecular weight of a chemical compound, it tells us how many grams are in one mole of that substance. The formula weight is simply the weight in atomic mass units of all the atoms in a given formula.
ConvertUnits.com provides an online conversion calculator for all types of measurement units. You can find metric conversion tables for SI units, as well as English units, currency, and other data. Type in unit symbols, abbreviations, or full names for units of length, area, mass, pressure, and other types. Examples include mm, inch, 100 kg, US fluid ounce, 6'3", 10 stone 4, cubic cm, metres squared, grams, moles, feet per second, and many more!