Joseph Marcus November 15, 2007 Chem 1AL Experiment 5 Discussion The goal of this experiment is to learn how to measure the volumes of gases and calculate the molar volumes of a gas a STP using the ideal gas law and Dalton’s law of partial pressures. We used the decomposition of hydrogen peroxide into water and oxygen gas to determine the amount of oxygen gas produced. The volume of the oxygen gas produced was equal to the volume of water that was displaced multiplied by (pressure recorded / pressure actual (760 torr)) multiplied by (temperature recorded / temperature actual (22 ° C., using the ideal gas law. The volume of the hydrogen gas is found in the same way. Part 1 The molar volume of O 2 at STP from the experiment is 22.197 L/mol. H 2 O 2 is decomposed in a closed beaker by a catalyst (FeCl 3 ) leaving behind H 2 O and O 2 gas. The oxygen gas escapes and passes through a rubber tube into another beaker filled with water. The displacement of water is measured and is recorded as the experimental volume
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This note was uploaded on 12/02/2009 for the course CHEM 1A taught by Professor Van koppen during the Spring '07 term at UCSB.