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Confirm Gas Laws . Prof. Cebula .

Introduction Gas molecules move at random and collide with each other unexpectedly. The distance between the molecules is largely dependent on the temperature the substance is at. Pressure, temperature, and volume are all related to gas expansion. Most gases function in the same way. The ideal gas law formula works for any gas at a lower density or a high temperature. Experimental Details For this experiment, I used the PhET “Gas Properties” lab from Colorado University Boulder. To begin the experiment, I had to confirm Boyle’s Law, PV= K I added 50 “light” molecules and changed the volume of the box while keeping the temperature constant. As the volume decreased, the pressure increased. As the volume increased, the pressure decreased. Initial (trial 1) Initial (trial 2) Final (trial 1) Final (trial 2) Pressure 2.4 atm 2.2 atm 6.2 atm 1.6 atm Volume (width) 15.0 nm 7.9 nm 5.0 nm 13.4 nm Boyle’s Law: PV= K Trial 1- Initial: (2.4 atm)(15.0 nm)= 36 Final: (6.2 atm)(5.0 nm)= 31 Trial 2- Initial: (2.2 atm)(7.9 nm)= 17.38 Final: (1.6 atm)(13.4 nm)= 21.44 This confirms Boyle’s law because the constants are very close. These numbers will not be exact because it is an experiment. Image 1. This image shows the end result of Boyle’s Law.

The next part of the experiment was to confirm Charles’ Law, V/T= K Once again, I added 50 “light” molecules and changed the volume of the box while keeping the pressure constant. As the temperature increased, the volume increased and vice versa. Initial (trial 1) Initial (trial 2) Final (trial 1) Final (trial 2) Temperature 58 K 124 K 95 K 178 K Volume (width) 8.6 nm 9.7 nm 14.0 nm 13.9 nm Charles’ Law: V/T= K Trial 1- Initial: (8.6nm)/(58K)= .15 Final: (14.0nm)(95K)= .15 Trial 2- Initial: (9.7nm)/ (124 K)= .08 Final: (13.9 nm)/ (178 K)= .08 This confirms Charles’ law because the constants are the same. Image 2. This picture shows the end result of Charles’ Law. The last part of this experiment was to confirm Gay-Lussac’s Law, PT= K I added 50 “light” molecules again and changed the temperature while keeping the volume constant. As the temperature was increased, the pressure also increased. Initial (trial 1) Initial (trial 2) Final (trial 1) Final (trial 2) Temperature 163 K 60 K 199 K 42 K Pressure 3.2 atm 1.4 atm 2.6 atm 2.0 atm Gay-Lussac’s Law: P/T= K Trial 1- Initial: (3.2 atm)/(166 K)= .0193 Final: (5.7 atm)/(294 K)= .0194

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