How many grams Lead(II) Carbonate in 1 mol?
The answer is 267.2089.

We assume you are converting between **grams Lead(II) Carbonate** and **mole**.

You can view more details on each measurement unit:

molecular weight of Lead(II) Carbonate or
mol

The molecular formula for Lead(II) Carbonate is PbCO3.

The SI base unit for **amount of substance** is the mole.

1 grams Lead(II) Carbonate is equal to 0.003742390317089 mole.

Note that rounding errors may occur, so always check the results.

Use this page to learn how to convert between grams Lead(II) Carbonate and mole.

Type in your own numbers in the form to convert the units!

Note that all formulas are case-sensitive.
Did you mean to convert one of these similar formulas?

grams PBCO3 to moles

grams PbCO3 to moles

grams PbCo3 to moles

grams PBCo3 to moles

1 grams Lead(II) Carbonate to mol = 0.00374 mol

10 grams Lead(II) Carbonate to mol = 0.03742 mol

50 grams Lead(II) Carbonate to mol = 0.18712 mol

100 grams Lead(II) Carbonate to mol = 0.37424 mol

200 grams Lead(II) Carbonate to mol = 0.74848 mol

500 grams Lead(II) Carbonate to mol = 1.8712 mol

1000 grams Lead(II) Carbonate to mol = 3.74239 mol

You can do the reverse unit conversion from moles Lead(II) Carbonate to grams, or enter other units to convert below:

grams Lead(II) Carbonate to decimol

grams Lead(II) Carbonate to molecule

grams Lead(II) Carbonate to atom

grams Lead(II) Carbonate to nanomol

grams Lead(II) Carbonate to kilomol

grams Lead(II) Carbonate to centimol

grams Lead(II) Carbonate to picomol

grams Lead(II) Carbonate to millimol

grams Lead(II) Carbonate to micromol

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.

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.

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.

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.

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.

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.

**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!