1. Illustrate the equation for photosynthesis.

Atomic Structure Chemical Bonding Chemical Reactions StoichiometrySolutions Acid/Base Chemistry Kinetic Molecular Theory

Learning Target: Identify and solve different types of stoichiometry problems by balancing chemical equations. By: Coach Lightfoot

 Stoichiometry: Calculations of quantities in chemical reactions. BALANCING EQUATIONS!  Indicates how much substance you end with based on how much you started with. ▪ A + 2B  AB 2 ▪ A 3 B 2 CD  3A + 2B + C + D ▪ A 2 + 3B 2  2AB 3 ▪ A 2 + B 2  2AB

 Atoms:  # of atoms in reactant = # of atoms in product.  Molecules:  # of molecules in reactant = # of molecules in product.  Moles: (1 dozen = ?; 1 pair = ?; 1 mole = 6.0 x )  A balanced equation indicates the # of moles in the reactants and products.  N 2 (g) + 3H 2 (g)  2NH 3 (g)  One molecule of N 2 reacts with three H 2 molecules to yield 2 molecules of NH 3.

1. N 2 (g) + H 2 (g)  NH 3 (g) 2. H 2 S(g) + O 2 (g)  SO 2 (g) + H 2 O(g) 3. CO 2 (g) + H 2 O(l)  C 6 H 12 O 6 (aq) + O 2 (g)

 Isoamyl acetate is the molecule found in banana flavor. In the production of banana flavor, so many molecules isoamyl acetate is produced that the molecule is also used to make air fresheners and artificial leather!

 Identify the reaction type of each reaction and balance. 1. H 2 + I 2  HI 2. Na + Cl 2  NaCl

 What is stoichiometry?  Explain the relevance of balancing equations.  How much is a mole?

 Read Section 12.1

 Indicate the reaction type, the amount of molecules and the amount of moles of each reactant and product:

Learning Target: Identify and solve different types of stoichiometry problems using units of moles and masses of reacting particles. By: Coach Lightfoot

 Used to convert moles to mass and mass to moles using mole ratios!

 The conversion factor derived from the coefficients of a balanced equation interpreted using moles.

 1 mole of H 2 WRONG!!!  1 mol of H 2 WRONG!  1 mol H 2 ALMOST!!!  1mol H 2 RIGHT!!!

 Converting moles to moles!  N 2 (g) + 3H 2 (g)  2NH 3 (g)  Calculate moles of NH 3 produced when 0.60mol N 2 reacts with H 2.

 Converting moles to mass!  N 2 (g) + 3H 2 (g)  2NH 3 (g)  Calculate number of grams of NH 3 (g) produced by the reaction of 5.40g of H 2 (g) with an excess of nitrogen.

 mA  nB

 5C(s) + 2SO2(g)  CS2(l) + 4CO(g)  Calculate moles of CS2 produced when 2.7mol C reacts.

 Moles can be converted to any other unit measurement related to the unit mole.

 Study your notes!!!

Learning Target: Indicate limiting reagents in chemical rxns and calculate percent yields. By: Coach Lightfoot

 Take 2min: What things are the most important to consider when cooking?  Limiting Reagent: Substance in chemical rxn that used up completely.  Rxn will proceed until the limiting reagent is used up.  Excess Reagent:…?

 Theoretical Yield: The amount of product that is calculated to be produced in a rxn.  Actual Yield: …?  Percent Yield: Ratio of actual yield and theoretical yield expressed as a percent.

 Percent yield is a measure of the efficiency of a rxn carried in the lab.  Ex. ▪ …  Take 2min: What factors can cause actual yield to be less than the theoretical yield?

 Read Section 12.3!  Test Friday!

Learning Target: By: Coach Lightfoot

 Limiting Reagent  Excess Reagent

Limiting ReagentExcess Reagent Reactant that’s being used up!Reactant that’s not being used up!

 Study for the Test!  Quizzes and Worksheets!

Theoretical YieldActual Yield Maximum amount of product that could be formed from given amounts of reactants. The amount of product that is actually formed when the rxn is carried out in the lab.