1 / 8

Gas Stoichiometry

Gas Stoichiometry. A balanced equation shows the ratio of moles being used and produced Because of Avogrado’s principle, it also shows the ratio of volumes being used and produced. Example. 2C 4 H 10(g) + 13O 2(g)  8CO 2(g) + 10 H 2 O (g) Shows molar and volume ratios Questions:

deiondre
Download Presentation

Gas Stoichiometry

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Gas Stoichiometry • A balanced equation shows the ratio of moles being used and produced • Because of Avogrado’s principle, it also shows the ratio of volumes being used and produced

  2. Example 2C4H10(g) + 13O2(g) 8CO2(g) + 10 H2O(g) • Shows molar and volume ratios • Questions: • How many moles of oxygen are required to produce 35 moles of water? • How many liters of butane does it take to completely react with 50 liters of oxygen?

  3. Try It • What volume of oxygen (O2) is needed to react with solid sulfur to form 3.5 L of SO2 gas? O2(g) + S(s) SO2(g) so 3.5 L O2 yields 3.5L SO2 • What volume of oxygen is needed to completely combust 2.36 L of methane gas? CH4(g) +2O2 (g)CO2(g) + 2H2O(g) 2.36 L CH4 X 2 mol O2/ 1 mol CH4 = 4.72 L O2

  4. Volume and Mass Problems • A balanced equation indicates both moles and volume (for gases) and can convert either to mass • Example: N2(g) + 3H2(g) 2NH3(g) If 5.00 L of nitrogen reacts completely at a constant pressure and temperature of 3.00 atm and 298 K, how many grams of ammonia are produced?

  5. Try It • Given: NH4NO3(s) N20(g) + 2H2O(g) Calculate the mass of solid ammonium nitrate that must be used to obtain .100 L of dinitrogen oxide gas at a pressure of 3.00 atm and a temperature of 15o C. Hints: change .100 L of N20 into moles calculate moles of NH4NO3 that reacted calculate the mass of the NH4NO3

  6. Answers • NH4NO3(s) N20(g) + 2H2O(g) PV = nRT or n = PV / RT n = 3.00 atm x .100 L / 288 K x .0821 atm.L/K.mol = .0127 mol N2O  .0127 mol NH4NO3 .0127 mol NH4NO3 x 79.035 g/mol = 1.00 g NH4NO3

  7. Try It 2. Solid potassium metal will react with Cl2 gas to form ionic potassium chloride. How many liters of Cl2 gas are needed to completely react with .204 g of potassium at STP? 2K(s) + Cl2(g) 2KCl(aq) Steps: convert grams of K into moles determine moles of Cl2 needed convert moles of Cl2 to liters

  8. Answers 2K(s) + Cl2(g) 2KCl(s) .204 g K x 1 mol / 39.098 g = .00522 mol K .00522mol K x 1 mol Cl2 / 2 mol K = .00261mol Cl2 PV = nRT so V = nRT/P = .00261mol Cl2 x .0821atm.L/K.mol x 273 K / 1.00 atm = .0585 L or 5.85 x 10-2 L or 58.5 ml

More Related