1. Chemical Reactions Unit 7 1

2. Chemical Equations 2 Combustion Reactions A substance reacts with O 2 (typically with the help of a flame) 2 C 4 H 10 + 13 O 2  8 CO 2 + 10 H 2 O The coefficients in chemical reactions can be interpreted as moles 2 moles of C 4 H 10 react to form 8 moles of CO 2 Conversion Factor!

3. Chemical Equations 3 2 C 4 H 10 + 13 O 2  8 CO 2 + 10 H 2 O 26 g of C 4 H 10 is combusted. How much water is formed (expressed in g) How much carbon dioxide is formed (expressed in g)

4. Chemical Equations 4 2 C 4 H 10 + 13 O 2  8 CO 2 + 10 H 2 O 26 g of C 4 H 10 is combusted. How much O 2 was consumed in the reaction? Is mass conserved? (does the mass of products = mass of reactants?

5. Chemical Equations 5 Sulfur dioxide (an environmental pollutant that leads to acid rain) is produced when sulfur containing fossil fuels are combusted. An example of this process is the unbalanced equation below: ZnS (s) + O 2 (g)  ZnO (S) + SO 2 (g) How much oxygen (in grams) is needed to completely react with 8.00 g of ZnS.

6. Chemical Equations 6 Sulfuric acid dissolves many metals. A product of this reaction is SO 2, the hazardous gas discussed in the previous example. Cu(s) + H 2 SO 4 (aq)  CuSO 4 (aq) + H 2 O(l) + SO 2 (g) How much SO 2 (in grams) can be produced from 18.00 g of Cu? How much sulfuric acid (in grams) is needed?