Gas Laws Worksheet (Chapter 5) Boyles Law: P1V1=P2V2 (Inverse Relationship) Charles’ Law: V1 T1 P = Pressure in atmospheres (atm) 1 atm = 760 torr = 760 mm Hg V2 T2 V = Volume in liters (L) (Direct Relationship) Combined Gas Law: P1 V1 T1 P2 V2 T2 Ideal Gas Law: PV=nRT Density of a gas : d mass vol. T = Temperature in Kelvin (K) n = Number of moles P( MW ) RT R = Ideal gas constant R = 0.082057 L(atm)/K(mol) Using the proper equations solve (complete) each question. Assume all are “ideal” gasses. 1. What is the pressure of a gas if you compressed the gas from its original 500 mL at 3.4 torr to a volume of 302 mL? 2. At what temperature will a gas be at if you allow it to expand from an original 456 mL at 65 qC to 3.4 L? 3. If you have 0.56 moles of an ideal gas at 87 qC and a pressure of 569 torr, what volume will the gas take up? 4. You have a gas at 453 mm Hg with a volume of 700 mL and a temperature of 25 qC, what will the temperature of the gas be, if you change the pressure to 278 mm Hg and a volume of 1200 mL? 5. Analysis of a gaseous chlorofluorocarbon, CClxFy, shows it contains 11.79 % C and 69.57 % Cl. In another experiment you find that 0.107 g if the compound fills a 458 mL flask at 25 qC with a pressure of 21.3 mmHg. What is the molecular formula of the compound?