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CHEM 1030 Cagg Chapter 8 Notes

by: Amy Notetaker

CHEM 1030 Cagg Chapter 8 Notes Chem 1030

Marketplace > Auburn University > Chemistry > Chem 1030 > CHEM 1030 Cagg Chapter 8 Notes
Amy Notetaker
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About this Document

These notes cover chapter 8 material. I only included sections 8.1, 8.1, and 8.4, since 8.3 was all math, and 8.5 will not be on the test.
Fundamental Chemistry I
Brett A Cagg
Class Notes
Cagg, CHEM 1030
25 ?




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This 2 page Class Notes was uploaded by Amy Notetaker on Wednesday April 6, 2016. The Class Notes belongs to Chem 1030 at Auburn University taught by Brett A Cagg in Spring 2016. Since its upload, it has received 23 views. For similar materials see Fundamental Chemistry I in Chemistry at Auburn University.


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Date Created: 04/06/16
Cagg Chapter 8 Notes Section 8.1 • Chemical reaction: a process that doesn’t create or destroy atoms. • Chemical equations: use symbols to tell what is happening in a chemical reaction. v Interpreting and Writing a Chemical Equation • Reactant: the chemical species that is on the left of the arrow. • Product: the chemical species that is on the right of the arrow. Products are what form in the process of a chemical reaction. • Aqueous: chemical species that are dissolved in water. • Metals in chemical equations: their empirical formulas are used to represent them. - Example: Iron would be “Fe” • Nonmetals in chemical equations: the molecular formula is generally used. - Example: Hydrogen would be “H ” ▯ • Noble gasses in chemical equations: the symbols are used. - Example: Argon would be “Ar” • Metalloids in chemical equations: their empirical formulas are used to represent them. - Example: Boron would be “B” v Balancing Chemical Equations • In a balanced equation, the same amount of one element must be on either side. • In order to balance, you write the correct amount of stoichiometric coefficients in front of the chemical formulas. • Law of conservation of mass: states that atoms cannot be created or destroyed. v Patterns of Chemical Reactivity • Combination reaction: a reaction in which 2 or more reactants combine to form one product. • Decomposition reaction: this is the opposite of combination. It is when a reaction that has 2 or more products that form a one reactant. • Combustion reaction: when a substance burns in the presence of oxygen. Section 8.2 • Combustion analysis: the experimental determination of the empirical formula. v Determination of Empirical Formula • You can determine the molecular formula of a compound if you know its mass. Section 8.4 • The goal of a reaction is to produce as much as you can of a compound from the materials you already have. Cagg Chapter 8 Notes • Limiting reactant: the reactant that is used up first, and limits the amount of more products from forming. • Excess reactants: extra reactants that are not used up. v Reaction Yield • Theoretical yield: calculating the amount of product formed in a reaction. This is the maximum yield. • Actual yield: the amount that is actually formed from a reaction. This is almost always less than the theoretical yield. • Percent yield: the formula that chemists use to determine the efficiency of a chemical reaction. - The formula for percent yield is ▯▯▯▯▯▯ ▯▯▯▯▯×100% ▯▯▯▯▯▯▯▯▯▯▯ ▯▯▯▯▯ - The percent yield outcomes cannot be greater than 100%


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