2. The Law of Conservation of Mass

3. We’ve talked about changes in matter… The evaporation of a puddle of water Rust forming on a metal fence PHYSICAL CHEMICAL

4. HOWEVER… No matter is created or destroyed by such changes! The total amount of matter remains constant.

5. The Law of Conservation of Mass During a chemical reaction, matter cannot be created or destroyed. Even though the matter may change from one form to another, the same number of atoms exists before and after the change takes place!

6. Since the overall mass of the matter does not change… The mass of the reactants – (the substances there before the reaction occurs) – must equal the mass of the product – (the substances there after the reaction takes place.) Mass of Reactants Mass of Products

7. Open System There is exchange of matter and energy with surroundings Mass is lost to the environment; once gone, that mass cannot be measured. Example: Burning Wood

8. Closed System No matter can enter/leave the system only energy

9. An Example of the Closed System. lead nitrate potassium iodideTest tube containing lead nitrate is placed upright in a flask that contains potassium iodide. What are these? –REACTANTS! They don’t mix!

10. A stopper is put in place to create a closed system – an environment where matter cannot enter or escape. The mass of the system is found.

11. After the mass is found, the system is turned upside down so the lead nitrate can mix with the potassium iodide. They create lead iodide and potassium nitrate.

12. Although the matter changed in form, the total mass of the system remains unchanged.

13. When iron reacts with oxygen in the air, they form rust or IRON OXIDE. This is written as: Iron + Oxygen Iron Oxide

14. Fe REACTANTS O2O2 O2O2 O2O2 PRODUCT Fe 2 O 3 TAKE A LOOK AT THE NUMBERS How many Iron molecules? How many Oxygen molecules? What about the PRODUCT?

15. All Chemical Reactions follow the Law of Conservation of Matter With Iron Oxide, the MASS STAYS THE SAME! –The total number of iron atoms and oxygen atoms in the reactants is the same as that in the product. –The atoms were just rearranged! No new atoms were created and none were destroyed!

16. Determining the Mass of Reactants and Products REMEMBER: The mass of the reactants is always equal to the mass of the products. Mass of Reactants Mass of Products

17. What are Chemical Equations A chemical change is represented by a chemical reaction. A chemical equation identifies the starting and ending chemicals as reactants and products: reactants  products

18. (c) McGraw Hill Ryerson 2007 Chemical reactions result in chemical changes. –Chemical changes occur when new substances are created. –The original substance(s), called reactants, change into new substance(s) called products. See pages 202 - 203

19. (c) McGraw Hill Ryerson 2007 See pages 202 - 203

20. (c) McGraw Hill Ryerson 2007 Chemical reactions can be written in different ways. –A word equation: Nitrogen monoxide + oxygen  nitrogen dioxide –A symbolic equation: 2 gg 2 g2NO (g) + O 2(g)  2NO 2(g) STATE OF MATTER - Letters indicate the state of each compound. (aq) = aqueous/dissolved in water (s) = solid ( ) = liquid (g) = gas COEFFICIENTS - Indicates how many of each molecule there is. -Ie: there are 2 molecules of NO.

21. (c) McGraw Hill Ryerson 2007 When a chemical reaction occurs, new compounds are created, BUT… –No new matter is created or destroyed rearrangedchange partners –No new matter is created or destroyed; atoms are just rearranged as the atoms change partners to form new compounds. 3 –If there are 3 atoms of oxygen in the reactants, there MUST be 3 atoms of oxygen in the products. –Number of each atom in reactants = number of each atom in products. The law of conservation of mass: –Mass of reactants = mass of products If you could collect and measure all of the exhaust from this car, you would find that mass of reactants (gas + O 2 ) = mass of products (exhaust).

22. The simplest form of chemical equation is a word equation. –Potassium metal + oxygen gas  potassium oxide A skeleton equation shows the formulas of the elements/compounds. –A skeleton equation shows which atoms are involved, but not how many molecules are involved. K + O 2  K 2 O

23. balanced chemical equation coefficientsA balanced chemical equation shows all atoms and the coefficients tells us how many molecules (and atoms) there are. ensures number of each atom same on both sides –Balancing ensures that the number of each atom is the same on both sides of the reaction arrow. 42 4K + O 2  2K 2 O K K K K K K K K K K K K K K K K OO O O

24. (c) McGraw Hill Ryerson 2007 count atoms to balanceUsing the law of conservation of mass, we can count atoms to balance the number of atoms in chemical equations. –Word equation: methane + oxygen  water + carbon dioxide –Skeleton equation:CH 4 + O 2  H 2 O + CO 2 To balance the compounds, take note of how many atoms of each element occur on each side of the reaction arrow. See Page 207

25. Balancing Equations CH 4 + O 2 H 2 O + CO 2 C C H H O O

26. Balancing Equations CH 4 + O 2 H 2 O + CO 2 C- 1 C -1 H - 4 H- 2 O - 2 O -3

27. Balancing Equations CH 4 + O 2 2 H 2 O + CO 2 C- 1 C -1 H - 4 H- 2 4 O - 2 O -3 4

28. Balancing Equations CH 4 + 2 O 2 2 H 2 O + CO 2 C- 1 C -1 H - 4 H- 2 4 O – 2 4 O -3 4

29. (c) McGraw Hill Ryerson 2007 Skeleton equation:CH 4 + O 2  H 2 O + CO 2 11 Carbon = 1Carbon = 1 42 Hydrogen = 4Hydrogen = 2 23 Oxygen = 2Oxygen = 3 22 11 Balanced equation:CH 4 + 2O 2  2H 2 O + CO 2 Carbon = 1Carbon = 1 44 Hydrogen = 4Hydrogen = 4 44 Oxygen = 4Oxygen = 4 The same number of atoms must be on each side. See Page 207

30. Balancing Equations ReactantsProducts H22 hydrogen + oxygen  water O 2 O 2  H2OH2OH2OH2O H 2 H 2 +O21

31. Balancing Equations H 2 + O 2  H 2 O 2 ReactantsProducts H22 O22 hydrogen + oxygen  hydrogen peroxide X YOU CANNOT CHANGE THE SUBSCRIPTS

32. Balancing Equations H 2 + O 2  H 2 O ReactantsProducts H22 O21 hydrogen + oxygen  water 2

33. Balancing Equations H 2 + O 2  H 2 O ReactantsProducts H24 O22 hydrogen + oxygen  water 2

34. Balancing Equations 2 2 H 2 + O 2  H 2 O ReactantsProducts H44 O22 hydrogen + oxygen  water 2 (g) (l)

35. http://www.youtube.com/watch?v=_B735turDoM

36. Balance the following: –Fe + Br 2  FeBr 3 –C 2 H 6 + O 2  CO 2 + H 2 O

37. ____Ba + ____H 2 O  ____Ba(OH) 2 + ____H 2 ____CO 2 + ____H 2 O  ____H 2 CO 3 ____Fe 2 O 3 + ____C  ____Fe + ____CO ____Fe + ____H 2 O  ____H 2 + ____Fe 2 O 3