# CHEM 06100 Lecture Notes - Lecture 3: Molar Mass, Unified Atomic Mass Unit, Stoichiometry

by OC1971726

School

Rowan UniversityDepartment

Chemical Engineering BiochemistryCourse Code

CHEM 06100Professor

GriniasLecture

3This

**preview**shows half of the first page. to view the full**1 pages of the document.**Stoichiometry and Chemical Reactions

• Stoichiometry- to determine how much mass, moles, and the making of product.

The mole (mol) if we take 12 grams of carbon 12 we have 1 mol.

One Mole (1mol) * 6.22x1023

Calculating Molar Mass

An Atom: Na= 1 x M of Na = 22.99g/ mol (amu)

A molecule molar mass:

O2= 2 x M of O = 2 x 16.00 g/mol = 32.00g/mol (amu)

H2O= 2 M of H= 2.00+ 1 MO= 16.00=18.00g/mol

An Ion (particle)= CI= 1 x < =35.45 g/mol

A formula Unit NaCl= 1 x M of Na = 22.99+1 x M of CI = 35.45 g/mol = 58.44g/mol

• Need a transfer electron and electronegativity to make Ion.

Mass Percent from the chemical formula

Mass % of elements x =

[ atoms of x in formula] x [ atomic mass of x (amu)]

Molecular (or formula) mass of compound (amu)

Mass of elements x=

[moles of x in formula]x [ molar mass of x(/mol 0]

Mass (g) of 1 mol of compound

Mass Fraction and the Mass of an Element

Mass of any element in sample

Mass of compound x mass of element in 1 mol of compound

Mass of 1 mol of compound

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