1. Quantitative Analysis

2.  Deals with mass relationships of elements in compounds Formula (molar) mass Converting grams to moles to atoms/molecules Find the molar mass of: Al 2 O 3 = Al = O 2 =

3.  Involves the mass relationships between reactants and products in a chemical reaction  Based on balanced chemical equations and the law of conservation of mass  Mole ratio = a conversion factor that relates the amounts in moles of any two substances involved in a chemical rxn

4. Amt (moles) of given → amt (moles) of unknown Ex. 2Al 2 O 3 → 4Al + 3O 2 The coefficients represent the mole ratios of all elements and compounds in a balanced equation. For every 2 moles of Al 2 O 3, you produce 4 moles of Al and 3 moles of O 2 EXAMPLE: How many moles of oxygen will be produced if you decompose 5.8 moles of aluminum oxide?

5. Amt of given →amt of unknown→mass of unknown 2Al 2 O 3 → 4Al + 3O 2 EXAMPLE: What was the mass of aluminum oxide decomposed if 5 moles of oxygen is produced? For every 2 moles of Al 2 O 3, you produce 4 moles of Al and 3 moles of O 2

6. Mass of given Moles of given Moles of unknown 2Al 2 O 3 → 4Al + 3O 2 If 150 grams of aluminum oxide is decomposed, how many moles of aluminum are produced?

7. Mass of given Moles of given Moles of unknown Mass of unknown 2Al 2 O 3 → 4Al + 3O 2 If 300 grams of aluminum oxide is decomposed, what is the mass of aluminum produced? You have just calculated the theoretical yield of this reaction.

8.  Theoretical Amount calculated based on balanced equation and starting amount of reactant  Actual Amount actually produced in the lab when the reaction is observed.

9.  Exact required amount of reactants based on equation?  Not realistic  We will run out of supplies of one of the reactants and have excess of the others

10. = the reactant that limits the amount of the products that can be produced (because we have a limited amt) Excess reactant = the substance that is NOT used up completely

11. Given: equation and masses of reactants Unknown: limiting reactant 1. Write and balance chemical equation 2. Convert masses (g) of reactants into moles of reactants using their molar masses 3. Multiply mole amount of each reactant by mole ratio to determine mole amount of products Whichever reactant produces the least of the product is the limiting reactant.

12. N 2 H 4 (l) + H 2 O 2 (l) → N 2 (g) + H 2 O (g) Which is the limiting reactant when 0.750 mol of N 2 H 4 is mixed with 0.500 moles of H 2 O 2 ?

13. Fe (s) + H 2 O (g) → Fe 3 O 4 (s) + H 2 (g) When 36.0 g of water is mixed with 67.0 g of iron, which is the limiting reactant?

14. After limiting reactant is identified, you can use it to determine theoretical yield  Use mole amount of limiting reactant and mole ratio of equation to determine how much product is produced (just like you did last week) g givenmol givenmol unknowng unknown

15. Zn (s) + S 8 (s) → ZnS (s) 2.00 mol Zn reacts with 1.00 mol of S 8  What is the limiting reactant?  How many moles of the product are produced (what is the theoretical yield)?

16. 2.40 mol of C react with 3.10 mol of steam  What is the limiting reactant?  Calculate theoretical yield of each product

17. When you can calculate the moles used or produced, you can always convert it into grams USING MOLAR MASS!!! When you are given the mass of something, you MUST FIRST convert it into moles (USING MOLAR MASS!!) before you can begin a problem Grams → Moles → Moles → Grams