Summer 2007 Ch 3

Summer 2007 Ch 3 - Chapter 3 Stoichiometry of Formulas and...

Info iconThis preview shows pages 1–10. Sign up to view the full content.

View Full Document Right Arrow Icon
Stoichiometry of Formulas and Equations Chapter 3
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
mole(mol) - the amount of a substance that contains the same number of entities as there are atoms in exactly 12 g of carbon-12. This amount is 6.022x10 23 . The number is called Avogadro’s number and is abbreviated as N. One mole (1 mol) contains 6.022x10 23 entities (to four significant figures)
Background image of page 2
Water 18.02 g CaCO 3 100.09 g Oxygen 32.00 g Copper 63.55 g One mole of common substances.
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Information Contained in the Chemical Formula of Glucose C 6 H 12 O 6 ( M = 180.16 g/mol) Oxygen (O) Mass/mole of compound 6 atoms 96.00 g Carbon (C) Hydrogen (H) Atoms/molecule of compound Moles of atoms/ mole of compound Atoms/mole of compound Mass/molecule of compound 6 atoms 12 atoms 6 moles of atoms 12 moles of atoms 6 moles of atoms 6(6.022 x 10 23 ) atoms 12(6.022 x 10 23 ) atoms 6(6.022 x 10 23 ) atoms 6(12.01 amu) =72.06 amu 12(1.008 amu) =12.10 amu 6(16.00 amu) =96.00 amu 72.06 g 12.10 g
Background image of page 4
Interconverting Moles, Mass, and Number of Chemical Entities Mass (g) = no. of moles x no. of grams 1 mol No. of moles = mass (g) x no. of grams 1 mol No. of entities = no. of moles x 6.022x10 23 entities 1 mol No. of moles = no. of entities x 6.022x10 23 entities 1 mol
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Sample Problem 3.1 Calculating the Mass and the Number of Atoms in a Given Number of Moles of an Element PROBLEM: (a) How many moles of C are in 315 mg of carbon?
Background image of page 6
Sample Problem 3.2 Calculating the Moles and Number of Formula Units in a Given Mass of a Compound PROBLEM: What is the mass in grams of 4.65 x 10 22 molecules of tetraphosphorous decaoxide?
Background image of page 7

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Mass % of element X = (moles of X in formula) (molar mass of X (g/mol)) Mass (g) of 1 mol of compound x 100 Mass percent from the chemical formula
Background image of page 8
Sample Problem 3.3 Calculating the Mass Percents and Masses of Elements in a Sample of Compound PROBLEM: (a) Calculate the mass % of N in ammonium nitrate.
Background image of page 9

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 10
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 05/31/2008 for the course CHEM 1111 taught by Professor Robertparson during the Spring '08 term at Colorado.

Page1 / 28

Summer 2007 Ch 3 - Chapter 3 Stoichiometry of Formulas and...

This preview shows document pages 1 - 10. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online