CHEM 1030 Cagg Chapter 8 Notes
CHEM 1030 Cagg Chapter 8 Notes Chem 1030
Popular in Fundamental Chemistry I
Popular in Chemistry
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.
Reviews for CHEM 1030 Cagg Chapter 8 Notes
Report this Material
What is Karma?
Karma is the currency of StudySoup.
You can buy or earn more Karma at anytime and redeem it for class notes, study guides, flashcards, and more!
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%
Are you sure you want to buy this material for
You're already Subscribed!
Looks like you've already subscribed to StudySoup, you won't need to purchase another subscription to get this material. To access this material simply click 'View Full Document'