1. Quantitative Chemistry: Stoichiometry Maggie Li Hannah Bensky Eugene Kyere Elton Luong

2. 1.4.1 Theoretical Yields 2Na + Cl 2 -> 2NaCl 5g Na -> ____g NaCl 5g Na 1mol Na 2mol NaCl 58.44g NaCl 1 22.99g Na 2mol Na 1mol NaCl

3. 1.4.2 Limiting/Excess Reactants 2Na + Cl 2 -> 2NaCl Limiting is the one used up first. Excess is the amount left over after the limiting reactant is used up.

4. 1.4.3 Percent Yields Predicted is what you should have gotten based on theoretical yield (1.4.1). Actual or experimental is what you got through physical experimentation.

5. 1.4.4 Avogadro’s Number Used to determine particles or atoms per mole as a conversion of any element. 6.022x10 23 atoms/particles X = 1 mol X

6. 1.4.5 Standard Volume 1mol X (g) = 22.4L X (g) Any element is subject to this in a gaseous state at STP (standard temperature and pressure).

7. 1.4.6 Combined Gas Law Where p = pressure, V = volume, and T = temperature (K)

8. 1.4.7 Ideal Gas Law

9. 1.4.8 Ideal Gas Graphs Where A = pressure or volume and B = temperature Where A = pressure and B = volume PV=nRT

10. For the following problems, use the equation given above. 1.Given 10g of water, how many grams of oxygen will be produced? 2.Which is the limiting reactant if 20g of each reactant is used? How many grams of the excess is left? 3.If 6 moles of carbon dioxide made 176.45g of organic matter, what is the percent yield? 4.Calculate the number of water atoms needed to make 12 moles of oxygen. 5.If 13 liters of oxygen is given off by a plant, how many grams of sugar was also produced? 6.The oxygen in the previous problem was trapped in an airtight container at STP. The pressure and temperature was then doubled. Assuming the water is vapor, what is the new volume? 7.Using the new water volume from the previous problem, calculate the number of moles if the temperature becomes 356K and the pressure becomes 0.5atm.