1. Chapter 6 Chemical Reactions Chemistry 101

2. Chemical Reactions Chemical change = Chemical reaction Substance(s) is used up (disappear) New substance(s) is formed. Different physical and chemical properties.

3. Chemical Reactions

4. Evidence for chemical reactions 1.Color changes 2.A solid is formed (precipitation) 3.Bubbles form (gas) 4.Heat (and/or flame) is produced, or heat is absorbed

5. A + B  C + D Reactants Products Chemical Reactions Chemical Equation

6. Chemical Reactions Products contain the same atoms as reactants. Rearrangement of atoms

7. Solid (s) Liquid (l) Gas (g) Aqueous (aq) Ca(OH) 2 (s) + 2HCl(g)  CaCl 2 (s) + H 2 O(l) Chemical Equation Physical States (forms)

8. Chemical equation gives us some information: 1.Identities of the reactants and products. 2.Relative amounts of the reactants and products. 3.Physical states of the reactants and products. 4.Stoichiometry Chemical Equation

9. Type of chemical reactions A + B  AB 1. Synthesis reaction (combination) 2H 2 + O 2  2H 2 O AB  A + B 2. Decomposition (analysis) 2NaCl  2Na + Cl 2 A + BC  AC + B 3. Single replacement reaction Fe + CuSO 4  FeSO 4 + Cu AB + CD  AD + CB 4. Double replacement reaction NaCl + AgNO 3  NaNO 3 + AgCl

10. 5. Combustion C 3 H 8 + 5O 2  3CO 2 + 4H 2 O + Heat AB + xO 2  yCO 2 + zH 2 O + Heat (Energy) Type of chemical reactions

11. Why balancing? Balance a chemical equation All chemical equations should be balanced.

12. Balance a chemical equation Low of conservation of mass Atoms are neither destroyed nor created. They shift from one substance to another.

13. Always double check! Balance a chemical equation 1.Begin with atoms that appear in only one compound on the left and right. 2.If an atom occurs as a free element, balance it last. 3.Change only coefficients (not formulas). C 3 H 8 (g) + O 2 (g)  CO 2 (g) + H 2 O(g) last

14. Balance a chemical equation C 3 H 8 (g) + 5O 2 (g)  3CO 2 (g) + 4H 2 O(g) 2C 3 H 8 (g) + 10O 2 (g)  6CO 2 (g) + 8H 2 O(g) 22 3C 3 H 8 (g) + 15O 2 (g)  9CO 2 (g) + 12H 2 O(g) 33 Lowest set of numbers

15. Examples for Balancing __ C 2 H 5 OH(l) + __ O 2 (g)  __ CO 2 (g) + __ H 2 O(g) __ PbCl 2 (aq) + __ K 2 SO 4 (aq)  __ PbSO 4 (s) + __ KCl(aq) __ CaC 2 (s) + __ H 2 O(l)  __ Ca(OH) 2 (s) + __ C 2 H 2 (g)

16. __ Fe(s) + ____ O 2 (g)  __ Fe 2 O 3 (s) Examples for Balancing __ Fe(s) + ____ O 2 (g)  __ Fe 2 O 3 (s) Notes: Always use the lowest possible integer numbers. If you get a fraction, multiply it out.

17. Examples for Balancing __ B 4 H 10 (g) + ____ O 2 (g)  __ B 2 O 3 (g) + __ H 2 O(g)

18. “Solid potassium reacts with water to form hydrogen gas and potassium hydroxide dissolved in solution.” Write and balance the chemical equation for this reaction. K(s) + H 2 O(l) → KOH(aq) + H 2 11 2 2 Examples for Balancing 2 1