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Do NOW. Please draw the Lewis Dot structure of NO 3 -1 and identify if it is a polar or nonpolar molecule. . Ideal Gas Law . STP. Standard Temperature and Pressure T = 273 K (0 °C) P = 1 atm. Ideal Gas Law. PV = nRT R = ideal gas constant . Ideal Gas Constant .

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  1. Do NOW Please draw the Lewis Dot structure of NO3-1 and identify if it is a polar or nonpolar molecule.

  2. Ideal Gas Law

  3. STP Standard Temperature and Pressure T = 273 K (0 °C) P = 1 atm
  4. Ideal Gas Law PV = nRT R = ideal gas constant
  5. Ideal Gas Constant R = 0.0821(L atm)/(mol K) R= 8.314 (L kPa)/(mol K) R = 62.4 (L mmHg)/(mol K)
  6. Example Calculate the number of moles of gas contained in a 3.0 L vessel at 3.00 x 102 K with a pressure of 1.50 atm. 0.18 mol
  7. Example What volume will an ideally behaving gas containing 1.00 mole of particles occupy at STP?
  8. If I have 17 moles of gas at a temperature of 340 K, and a volume of 88.89 liters, what is the pressure of the gas?
  9. If I have 1.9 moles of gas held at a pressure of 5 atm and in a container with a volume of 50 liters, what is the temperature of the gas?
  10. Gas Stoichiometry 2C4H10(g) + 13O2(g)  8CO2(g) + 10H2O(g) What type of reaction is this? How many moles of butane gas react with how many moles of oxygen gas?
  11. Gas Stoichiometry 2C4H10(g) + 13O2(g)  8CO2(g) + 10H2O(g) Avogadro’s Principle: = V of gas at same T & P contain = # of particles  Coefficients represent not only molar amounts, but also relative volumes
  12. Gas Stoichiometry- Volume Only CH4(g) + 2O2(g)  CO2(g) + 2H2O (g) It takes 2 L of O2 to react completely with 1 L of CH4 The complete combustion of 1 L of methane produces 1 L of carbon dioxide and 2 L of water vapor. What volume of methane is needed to produced 26 L of water vapor?
  13. Gas Stoichiometry- Volume Only What volume of oxygen gas is needed for the complete combustion of 4 L of propane gas? Assume constant pressure and temperature. C3H8(g) + 5O2(g)  3CO2(g) + 4H2O(g) 20.0 L O2
  14. Gas Stoichiometry- Volume & Mass Balanced chemical equations allow you to find ratios for moles and volume – not for masses!
  15. Gas Stoichiometry- Volume & Mass N2(g) + 3H2(g)  2NH3(g) If 5.00 L of nitrogen reacts completely by this reaction at a constant pressure and temperature of 3.00 atm and 298 K, how many grams of ammonia are produced? Givens: VN2 = 5.00 L P = 3.00 atmT = 298 K Unknown: mNH3 = ?
  16. N2(g) + 3H2(g)  2NH3(g) Find VNH3. Rearrange Ideal Gas Law equation to solve for n. Convert moles of ammonia to grams.
  17. N2(g) +3H2 (g)→ 2NH3(g) What volume of nitrogen at STP would be required to react with 0.100 mol of hydrogen to produce ammonia?
  18. 4Fe(s) + 3O2(g)  2Fe2O3(s) Calculate the volume of oxygen gas at STP that is required to completely react with 52.0 g of iron. Convert Fe mass to moles. Determine number of moles of O2. Determine volume of O2 using Ideal Gas Law. Givens: mFe= 52.0 g T = 273 K P = 1 atm 15.6 L Unknown: VO2= ?
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