Download presentation
Presentation is loading. Please wait.
Published byLisa Webster Modified over 9 years ago
1
Chem Catalyst 1) Balance the following: Cu(s) + S(s) Cu 2 S(s) Be(s)+ O 2 (g) BeO(s) K(s) + Cl 2 (g) KCl(s) 2) What do these equations have in common?
2
Today’s Agenda: 1. Catalyst 2. Notes: Types of Chemical Reactions 3. Reaction analogies 4. P. 339 #24
3
Unit 5: Chemical Reactions BIG Questions 1. How does a chemical equation represent a chemical reaction? 2. Why do chemical reactions occur? 3. Why is balance essential when working with chemical reactions?
4
Combination (Synthesis) - Two or more substances combine to form a single compound - A + B AB - 2 Reactants, 1 Product - Ex: 2 Zn + O 2 2 ZnO
5
Decomposition Reaction - A single compound splits into two (or more) substances - XY X + Y - 1 Reactant, 2 Products - Ex: 2HgO (s) 2Hg(l) + O 2 (g)
6
Single-Replacement Reaction - An element replaces one of the ions in an ionic compound - A + BC AC + B - 2 Reactants, 2 Products - Ex: Cu(s) + AgNO 3 (aq) Ag(s)+ CuNO 3 (aq)
7
Double-Replacement Reaction - Ionic compounds exchange cations to form new ionic compounds - AB + XY AY + XB - 2 Reactants, 2 Products - Ex: FeCl 3 + 3 NaOH Fe(OH) 3 + 3 NaCl
8
Combustion - A hydrocarbon reacts with oxygen to form carbon dioxide and water - C x H y O z + O 2 CO 2 + H 2 O - 2 Reactants (hydrocarbon & O 2 ), 2 Products (CO 2, H 2 O) - Ex: C 2 H 5 O (l) + O 2 (g) CO 2 (g) + H 2 O (l)
9
Examples: 2 C 8 H 18 (l) + 25 O 2 (g) 16 CO 2 (g) + 18 H 2 O (l) 2HgO(s) 2Hg(l)+ O 2 (g) CaI 2 + Hg(NO 3 ) 2 HgI 2 + Ca(NO 3 ) 2 2Mg + O 2 2MgO Fe(s) + Pb(NO 3 ) 2 (aq) Pb(s) + Fe(NO 3 ) 2 (aq)
Similar presentations
© 2025 SlidePlayer.com. Inc.
All rights reserved.