chem notes 9-19 - September 19, 2007 Dr. Stevens Gen. Chem....

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
September 19, 2007 Dr. Stevens Gen. Chem. 1 Notes: -3.1 due Fri. 9pm -Exam 1 next Wed. -Review next Tuesday 9pm -Practice Exam on Bb Chapter 3 Objectives: -Determine mass of a mole in amu or of a mol in grams -Use Avogadro’s # to determine # of particles present -Interconvert between % composition and formula of a mole -balance chemical equations -use stoichiometry to determine masses of substances in a reaction Molar Mass (MM) -1 mol X = __ g X -__ g X/1 mol X = MM -Molar Mass of Compound: addition of all elements in the formula -MM(CH4) = 1xMM(C) + 4xMM(H) = 1(12.01) + 4(1.0079) = MM(CH4) = 16.04 g/mol -Can relate to # particles (mole) by Avogadro’s # mass <-> mol (varies) -through PT mol <-> particles (always the same) -Avogadro’s #: 6.022x10^23 -How many molecules are in 10.0 g CH4? -10.0g CH4 x 1 mol/16.04g x 6.022x10^23 mole/1 mol = 3.75x10^23 -If you have 10.0g Fe that rusts to form 0.0895 mol of Fe2O3, calculate total m of Fe2O3. -10.0g Fe + O2 = Fe2O3
Background image of page 1

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

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 2

chem notes 9-19 - September 19, 2007 Dr. Stevens Gen. Chem....

This preview shows document pages 1 - 2. Sign up to view the full document.

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