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Chapter 10 – Introduction to Equations

Chapter 10 – Introduction to Equations. Writing and Balancing Equations Section 10.1. Chemical Reactions. One or more substances are rearranged to form different substances C 8 H 18 + O 2 -> CO 2 + H 2 O + ENERGY LOOK, IT’S A HYDROCARBON!!!!! The products are carbon dioxide and water!.

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Chapter 10 – Introduction to Equations

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  1. Chapter 10 – Introduction to Equations Writing and Balancing EquationsSection 10.1

  2. Chemical Reactions • One or more substances are rearranged to form different substances C8H18 + O2 -> CO2 + H2O + ENERGY LOOK, IT’S A HYDROCARBON!!!!! The products are carbon dioxide and water!

  3. Indicators of Chemical Reactions • Animation of Experiment (GIF Format, 321 k) • Temperature Change • Color Change • Odor • Production of Gas Bubbles • Production of a Precipitate

  4. Representing Chemical Reactions • Statements called equations are used to describe what happens during a chemical reaction • Reactantsare the starting substances found on the left side of the equation • Products are the substances formed during a reaction

  5. Word Equations -Statements that indicate the reactants and products in a rxn -Describe chemical reactions -Lack important information Iron (s) + chlorine (g) -> iron (III) chloride (s) Skeleton Equations -Uses chemical formulas to identify reactants and products Fe (s) + Cl2 (g) -> FeCl3(s) Word Equations and Skeleton Equations

  6. Practice Problems Write skeleton equations for the following word equations: 1. hydrogen (g) + bromine (g) -> hydrogen bromide (g) H2(g) + Br2(g) -> HBr (g) 2. carbon monoxide (g) + oxygen (g) -> carbon dioxide (g) CO (g) + O2(g) -> CO2(g) 3. potassium chlorate(s) -> potassium chloride(s) + oxygen(g) KClO3(l) -> KCl (s) + O2(g)

  7. Balancing Equations Chemical Equations also must obey the Law of Conservation of Mass. The number of atoms that are used in the reactants must equal the number of atoms found in the products. Matter can neither be created nor destroyed. A chemical equation that follows the law of conservation of mass is called a balanced chemical equation. A Chemical Equation H2 + O2 -> H20 A Balanced Chemical Equation Coefficient… -> 2H2 + O2 -> 2H2O

  8. Balancing Chemical Equations There is a procedure for balancing chemical equations: • Write the equation (remember your diatomic molecules) • Count the atoms of each element • Add or adjust the coefficients (subscripts cannot be changed) • Reduce coefficients to lowest possible terms • Check your work Hydrogen + Chlorine Yields Hydrochloric Acid H2 + Cl2 -> HCl

  9. Balancing Equations Practice Al + O2 -> Al2O 4Al + O2 -> 2Al2O C3H8 + O2 -> CO2 + H2O C3H8 + 5O2 -> 3CO2 + 4H2O KNO3 -> KNO2 + O2 2KNO3 -> 2KNO2 + 2O2 O2 + CS2 -> CO2 + SO2 3O2 + CS2 -> CO2 + 2SO2

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