Notes

Unit 6 - Covalent Bonds



Chapter 9 - Gas Laws View these pages for Demonstrations: [|Boyle's Law] [|Charles' Law] [|Pressure & Moles in Ideal Gas] [|Volume & Moles in Avogadro's Law]

3/9/09

1) Converting to liters when a gas is at STP (standard temperature & pressure): 22.4 L/ 1 mol

2) Converting to liters when the molarity is given (M = mol/L) be sure to keep the # with moles. ex: 6 mol/ 1 L

3) Converting to molecules or atoms: 6.022 x 10²³ molecules

4) Using density: g/mL

3/16/09

__Determining the Amount of Excess Reactant Leftover__ From the worksheet on Thursday and Friday: We started with 10.0 grams of C 3 H 8 and 10.0 grams of O 2. This reaction formed 4.51 grams of H 2 O and 8.25 grams of CO 2. Oxygen was the limiting reactant and propane the excess reactant. C 3 H 8 + 5O 2 --> 3 CO 2 + 4 H 2 O

1) Pick one of the products to use as your starting number. 2) Use factor labeling to convert the grams of product into grams of excess. (This tells you how much excess was used.) 3) Subtract the amount of excess used from the starting material. (This tells you how much is left over.)



Excess Leftover: 10.0 g - 2.76 g = 7.74 g leftover Explore Learning: Limiting Reactants 1) Slide scale to decide how many of each reactant you want to mix. 2) Hit the play button under the molecules to watch the bonding occur. 3) When you see "reaction complete" observe the equation to see how many bonds are formed, what molecules was fully used, and which molecule is the excess. 4) Repeat with a few different combinations of each equation. 5) Complete the 5-question quiz when you're done. (you may need to use factor labeling to answer the questions)