CH301 - chapter 3 notes

CH301 - chapter 3 notes - 1 CH 301 Chapter 3 - Reading...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon
1 CH 301 Chapter 3 -- Reading Assignment 3-1 Chemical Equations (Do exercises 4 – 7 at the end of the chapter) Chemical equations are used to describe chemical reactions. Chemical equations have three parts: 1. Reactants and Products 2. States abbreviations (denoting the states in which the reactants and products exist) 3. The equation must be balanced (the Law of Conservation of Matter and Energy) Symbolic representation of a chemical reaction shows: 1. reactants on left side of reaction 2. products on right side of equation 3. relative amounts of each using stoichiometric coefficients Chemical equations attempt to show on paper what is happening at the laboratory and molecular levels. Chemical equations provide very useful information: E.g. reactants yields products 1 formula unit 3 molecules 2 atoms 3 molecules 1 mole 3 moles 2 moles 3 moles 159.7 g 84.0 g 111.7 g 132 g Law of Conservation of Matter ± There is no detectable change in quantity of matter in an ordinary chemical reaction. ± Balanced chemical equations must always include the same number of each kind of atom on both sides of the equation. ± This law was determined by Antoine Lavoisier. 23 2 Fe O + 3 CO 2 Fe + 3 CO →
Background image of page 1

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

View Full DocumentRight Arrow Icon
2 Example: Propane,C 3 H 8 , burns in oxygen to give carbon dioxide and water. Example: Solid P 4 will react with chlorine gas to produce solid PCl 5. P 4 (s) + Cl 2 (g) Æ PCl 5 (s) Example: Solid iron (III) oxide will react with gaseous carbon monoxide to produce gaseous carbon dioxide and iron metal. Fe 2 O 3 (s) + CO (g) Æ CO 2 (g) + Fe (s) Example: Aqueous sodium sulfate will react with aqueous lead (II) nitrate to produce solid lead (II) sulfate and aqueous sodium nitrate. Na 2 SO 4 (aq) + Pb(NO 3 ) 2 (aq) Æ PbSO 4 (s) + NaNO 3 Example: NH 3 burns in oxygen to form NO & water Example: Gaseous butane (C 4 H 6 ) will undergo combustion with atmospheric oxygen to produce gaseous carbon dioxide and water vapor. C 4 H 6 (g) + O 2 (g) Æ CO 2 (g) + H 2 O (g) 3-2 Calculations Based on Chemical Equations (Stoichiometry) (Do all even exercises, 8-24, and 19, 21, 23, and 25) From a balanced equation we can determine the amounts of reactants or products that would theoretically be used or produced during a chemical reaction:
Background image of page 2
Image of page 3
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 06/19/2008 for the course CH 301 taught by Professor Fakhreddine/lyon during the Spring '07 term at University of Texas at Austin.

Page1 / 7

CH301 - chapter 3 notes - 1 CH 301 Chapter 3 - Reading...

This preview shows document pages 1 - 3. Sign up to view the full document.

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