IdealGas_LabReport

# A syringe was connected to the pressure sensor at a

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relationship was verified using a pressure sensor in which the volume was varied. A syringe was connected to the pressure sensor at a volume of 10.0mL, and then pressure data was generated for 6 volumes. Pressures were recorded at the volumes indicated. The syringe was disconnected and adjusted to 5mL before reconnecting to the pressure sensor. The pressure at 5mL was recorded and then increased to 10mL and then to 20mL recording the pressure at each volume. Then this was repeated but starting at 20mL and adjusting to 10mL, always recording the pressure at the volume.

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Analysis: In the first part of the experiment after the student had gathered all the data set need, they converted the temperature to Kelvin, the barometric pressure to atmospheres, volume to liters, and using the molecular weight for CO 2 converted to moles in order to use these numbers in the ideal gas law to find the ideal gas constant R at each trial. The percent error was calculated with the equation given and using the mean values for the dry and wet ice trials. In the second part of the experiment the Overall mass of the butane was the subtraction of the final minus the initial weight of the lighter. The partial pressure of water was looked up and then was subtracted form the barometric pressure to find the pressure of butane. Again the temperature, pressure, and volume were converted to the appropriate units. These numbers were then used in the ideal gas law to solve for n, which was then divided into the mass of butane to get the molecular weight. The average
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