›› Convert moles Vanadium to gram

moles Vanadium

›› More information from the unit converter

How many moles Vanadium in 1 grams? The answer is 0.019630360315264.
We assume you are converting between moles Vanadium and gram.
You can view more details on each measurement unit:
molecular weight of Vanadium or grams
The molecular formula for Vanadium is V.
The SI base unit for amount of substance is the mole.
1 mole is equal to 1 moles Vanadium, or 50.9415 grams.
Note that rounding errors may occur, so always check the results.
Use this page to learn how to convert between moles Vanadium and gram.
Type in your own numbers in the form to convert the units!

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Convert moles to grams  

›› Quick conversion chart of moles Vanadium to grams

1 moles Vanadium to grams = 50.9415 grams

2 moles Vanadium to grams = 101.883 grams

3 moles Vanadium to grams = 152.8245 grams

4 moles Vanadium to grams = 203.766 grams

5 moles Vanadium to grams = 254.7075 grams

6 moles Vanadium to grams = 305.649 grams

7 moles Vanadium to grams = 356.5905 grams

8 moles Vanadium to grams = 407.532 grams

9 moles Vanadium to grams = 458.4735 grams

10 moles Vanadium to grams = 509.415 grams

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You can do the reverse unit conversion from grams Vanadium to moles, or enter other units to convert below:

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›› Common amount of substance conversions

moles Vanadium to micromol
moles Vanadium to molecule
moles Vanadium to millimol
moles Vanadium to kilomol
moles Vanadium to nanomol
moles Vanadium to mole
moles Vanadium to picomol
moles Vanadium to atom
moles Vanadium to decimol
moles Vanadium to centimol

›› Details on molecular weight calculations

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.

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.

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.

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.

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.

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.

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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!