Chapter 3

Chapter 3 - CHAPTER 3:- STOICHIOMETRY Study of quantities...

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

View Full Document Right Arrow Icon
CHAPTER 3:- STOICHIOMETRY Study of quantities of matter consumed and produced in a chemical reaction; based on law of Conservation of Mass Atomic masses: - Measurement of mass is relative; 12 C atom si reference for atomic masses (mass of 12 C is defined as exactly 12 amu - Measured via mass spectrometer - Atomic masses listed on the periodic table are the weighted average (Cr is NOT exactly 52.00) - To calculate atomic mass, know amu + abundance (percentage) of each isotope 2NaClO 3 + H 2 SO 4 Na 2 SO 4 + 2HClO 3 sodium sulfuric sodium chloric chlorate acid sulfate acid 8NaClO 3 + sucrose 8NaCl + 12CO 2 + 11 H 2 O 2KI + MnO 2 + 3H 2 SO 4 I 2 + MnSO 4 + 2KHSO 4 + 2H 2 O Amu = grams (average mass of 1 atom = average mass of 1 mole atoms) Mole (mol): # atoms in 12g pure 12 C; 6.022 x 10 23 Example: mass of 13 atoms Rh 13 atoms Rh x (1 mol Rh // 6.022 x 10 23 atoms Rh) x (102.9g Rh // 1 mol Rh) = 2.221 x 10 -21 g Rh Molar Mass: mass of one mole of compound (older term MOLECULAR WEIGHT);
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 11/18/2011 for the course CHEM 105ALg taught by Professor Bau during the Spring '07 term at USC.

Page1 / 3

Chapter 3 - CHAPTER 3:- STOICHIOMETRY Study of quantities...

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