Chapter 3 - Chapter 3: Mass and Moles of Substance and...

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

View Full Document Right Arrow Icon
Chapter 3: Mass and Moles of Substance and Determining Chemical Formula Pg. 87 - 102 I. Mass a. Atomic Mass (based on C-12) b. Oddities in the increasing trend i. Ar is heavier than K ii. Co is heavier than Ni 1. Each element has isotopes, so Ar abundant isotope is heavier than abundant isotope of K II. Molar mass (g/mol) a. 6.0221367 x 10 23 particles in one mole i. Avogadro’s number (N A ) III. Molecular Mass a. H 2 O = 2(1.008 g) + (15.994 g) = 18.01 g/mol IV.Formula Mass a. Sum of each element i. NaCl = 22.99 g + 35.45 g = 58.44 g/mol V. Determining Chemical Formula a. Percent composition – (mass % of each element) b. Empirical Formula – formula unit for ionic substances c. Molecular mass – for molecules i. Mass spectrometry d. Molecular formula VI.Elemental Analysis (Organic Compounds) a. To find % composition of C, H, O VII. Mass Percentage a. Mass % A = [(mass A in whole)/(mass of whole)] x 100 b. Ethanol C 2 H 6 O i. Mass % C = 24.02 (g/mol)/46.08 (g/mol) = 52.14 % c. Do combustion reaction to find percentages
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.

This note was uploaded on 01/27/2011 for the course CHEM 0310 taught by Professor Brummond during the Fall '08 term at Pittsburgh.

Page1 / 2

Chapter 3 - Chapter 3: Mass and Moles of Substance and...

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