1. Reaction Mole Ratios Set up ratios to show mole proportions in a balanced equation. Predict the amount of product produced when given the mass of the reactants. Predict the amount of reactants necessary to produce a desired amount of product.

2. Aim: How can we use mole ratios to predict the amount of products or reactants? Essential Questions: 1.How can we show mole proportions in a balanced equation? 2.How do we predict the amount of products produced given the amount of reactants. Use examples to illustrate your answer. 3.How can we calculate the amount of reactants needed when given the amount of product? Use examples to illustrate your answer. Key Words: Gram formula mass, mole ratio, chemical equation, reactant, product

3. Do Now Balance the following chemical reactions and indicate the type of reaction for each equation Balance the Following EquationsType of Reaction ___ CaCO 3  ___ CaO + ___ CO 2 _________________ ____ Pb + ____ H 3 PO 4  ____ H 2 + ____ Pb 3 (PO 4 ) 2 _________________

4. Our Chemistry Class is Out Camping!  _____ + + ____ Gc + ____ M + ____ Cb  ____ Gc 2 MCb

5. Air Bags For an airbag to deploy an exact quantity of nitrogen gas must be produced in an instant. 2 NaN 3 (s)  2 Na(s) + 3 N 2 (g)

6. To Predict the Amount of Product or Reactants. 1.Find the formulas for each compound and write the equation. 2.If anything is written in terms of grams, convert it into moles immediately. 3.Set up ratios to show mole proportions based on what is given and what needs to be found. 4.Work through the ratios to find the answer in moles. 5.Convert the answer into grams if necessary.

7. Solve This! In the decomposition reaction of hydrogen peroxide to form water and oxygen, how many grams of hydrogen and how many grams of oxygen can be made from the decomposition of 17 grams of hydrogen peroxide?

8. Homework Complete the sheet that is given out to you today! Also, remember to complete the review sheet because we will go over the questions tomorrow!

9. Group Work A.) In a reaction of iron metal with oxygen to form iron (III) oxide, how many moles of oxygen are needed to make 100 grams of iron (III) oxide? How many grams of iron are needed? B.) How many grams of hydrogen gas are needed to make 1 mole of copper metal in a reaction between copper (II) oxide and hydrogen which forms copper metal and water?

10. Essential Questions: 1.How can show mole proportions in a balanced equation? 2.What are products and reactants? 1.How do we calculate the amount of products produced when given the mass of the reactants? Use examples to illustrate your answer.