Was removed from the bag afterwards and the bag was

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was removed from the bag afterwards and the bag was filled with water to as full as it had been with the CO 2 gas to measure the volume, recorded as CO 2 volume. The students recorded the barometric pressure that was provided by the instructor. The students converted all measurements to units used in the ideal gas law, and using measurements and barometric pressure given were able to calculate the ideal gas constant R. The mean value for the dry ice and wet ice were recorded and compared. In order to calculate the percent error (true value being 0.0821L-atm/k-mol): Percent Error = [(true value) - (experimental value)/ (true value)] * 100. In the second part the butane lighter was used to find the molecular weight of the gas. The students filled the buret with water and inverted it so that the buret end was under the water level. The room temperature RT was recorded and the water temperature in the beaker WT. The mass of the butane lighter was recorded on an analytical balance as the M i . A tube was attached to the butane outlet on the lighter and the other end was placed under the open buret barrel. The valve was pressed to release the butane gas into the buret until 35-45mL of gas had been obtained. The volume of the gas was recorded as V g . The tubing was removed, lighter was dried and reweighed and the mass was recorded, M f . Then the students repeated this process twice more to get three sets of data. The last part of the experiment the pressure/volume relationship was verified using a pressure sensor in which the volume was varied. A
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  • Spring '13
  • KarenAtkinson
  • pH

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