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Chapter 3

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

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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);

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

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