Experiment 5 - The calculated volume for experiment two,...

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Experiment 5 The Molar Volume of Gases The purpose of this experiment was to determine the molar volume of a gas and to learn how to measure the volumes of gases and calculate the molar volume at STP using the ideal gas law and Daltons law of partial pressures. Since we already know the molar volume is 22.4L, the idea was to get a value close to that number. This gas was collected in a sealed container, which was connected to a beaker with a hose. As the gas entered the flask, it displaced water which flowed through the hose and into the beaker. This amount of water was displaced was equal to the volume of gas produced. From this number, calculations were made to determine the molar volume of the gas, using the ideal gas law. The calculated molar volume for experiment one, which was oxygen, was 1.35 L/mol.
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Unformatted text preview: The calculated volume for experiment two, which was for hydrogen, was 29.1 l/mol. It is assumed that there is greater error in experiment two due to the higher difference between the calculated and expected value. This could be due to a number of reasons. The system for collecting gas could have had a leak, which would give result in less gas and increase the value for molar volume. Also there could have been error in measuring the mass and volume of the reactants to produce hydrogen gas. One way of correcting there errors would be to leak test the system and be very careful in measuring and collecting the data. Part 1 reaction: 2FeCl 3 (aq) + H 2 O 2 (aq) 2FeCl 2 (aq) + 2HCl (aq) + O 2 (g) Part 2 reaction: Mg (s) + 2HCL (aq) MgCl 2 (aq) + H 2 (g)...
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This note was uploaded on 04/20/2010 for the course CHEM1A/1B Chem Labs taught by Professor Van koppen during the Spring '10 term at UCSB.

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