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11.3 The Ideal Gas Law POINT > Review the Gas Laws POINT > Use KMT to explain how different gases occupy the same volume POINT > Show that equation coefficients can indicate gas volumes POINT > Define the Ideal Gas Law POINT > Review the Gas Laws Boyle’s Law: P1V1 P2V2 Charles’ Law: V1 V2 T1 T2 Combined Gas Law: (Units MUST match and temperature in Kelvin!) P1V1 P2V2 T1 T2 POINT > Review the Gas Laws A gas with a volume of 350. ml is collected at 15.0o C and 120. kPa. If the temperature changes to 30.0o C, what pressure would be required to put this gas in a 300. ml container? 120kPa 350ml P2 300ml 288K 303K P2 147.3kPa WB CHECK: A balloon has a volume of 500. ml at a temperature of 22.0oC and a pressure of 755 mmHg. If the balloon is cooled to 0.00o C and a pressure of 145 mmHg, what is its new volume? 755mmHg 500ml 145mmHg V2 295K 273K 2410 ml V2 POINT > Use KMT to explain how different gases occupy the same volume KMT tells us that gas particles, regardless of size, do not interact with each other Gay-Lussac noticed a volume relationship: 2 liters of H2 gas combined with 1 liter of O2 gas to form 2 liters of H2O vapor... POINT > Use KMT to explain how different gases occupy the same volume Here is the balanced equation: 2 H2 + O2 2 H2O The volume ratios of reactant and product gases were always small whole numbers (Gay-Lussac) Avogadro: At the same temperature and pressure, a defined volume of any gas has the same number of particles (At STP 1 mole of gas = 22.4L) POINT > Show that equation coefficients can indicate gas volumes If the reactants and products are gases, then the equation coefficients can indicate moles or volumes (Why?) One mole of any gas has the same number of particles (Avagadro’s number) The same number of particles of any gas occupy the same volume Stoichiometry can extend to gas volumes, as well as moles WB CHECK: 2 C4H10 + 13 O2 8CO2 + 10 H2O If 4.00 L of butane are combusted, how many L of water vapor could be produced? If 36.0 L of CO2 is produced during the above reaction, how much O2 was used? 58.5 L POINT > Define the Ideal Gas Law KMT tells us that pressure, temperature, and volume will all be affected by the number of gas particles This leads to the Ideal Gas Law: PV = nRT POINT > Define the Ideal Gas Law PV = nRT n = number of moles R = .0821 the gas constant if using atm, liters, and Kelvin as units If not using these units, convert to them or use a different R (Figure 3.4 p. 364) WB CHECK: PV = nRT Given 3 of the values, calculate the unknown quantity: How many moles of gas are contained in 890.0 mL at 21.0 °C and 750.0 mm Hg pressure? ~ 0.036 moles Hint: If the problem involves # of moles or mass, you must use the Ideal Gas Law to solve! WB CHECK: A 50.0L container of methane at STP contains how many moles of methane? 50.0L x 1 mole = 2.23 mol methane 22.4 L WB CHECK: At STP, what volume would 5.50 moles of water vapor occupy? 5.50mol x 22.4L 1 mol = 123L water vapor Homework: Read pages 358-365 7 Practice problems 358-365 FA #1-6 Page 365