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by: Devin Petit

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# lecture notes

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Devin Petit
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This 2 page Class Notes was uploaded by Devin Petit on Tuesday July 26, 2016. The Class Notes belongs to at Duquesne University taught by in Summer 2016. Since its upload, it has received 5 views.

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Date Created: 07/26/16
Name: Devin Petit  Date: 10/21 TA name: Riley Workman  Section: 04 Analysis of Gas Behavior Discussion Paragraph:  Write a paragraph containing comments on the results from the Lab “Analysis of Gas Behavior.” Please address the questions below. For full credit you must be specific in your answers and you  must answer in paragraph for.  (1) Did the experiment work? (2) Were the results expected? (3) If the experiment were to be repeated, what improvements on the procedure would be made? (4) If the experiment did  not work, Explain? (5) Possible explanations of any error that may have occurred.  The first part of the experiment, which tested the relationship of pressure in volume  presented in Boyle’s Law, was effective. The experiment fulfilled the purpose of discovering the  relationship between volume and pressure. The results showed that as the volume of the plunger  decreased, the total pressure exerted increased. For example, at 50 mL the total pressure was  15.295 lbs/in^2, but at 10 mL the totally pressure was 27.520 lbs/in^2. These results were  expected because Boyle’s Law states that volume of a gas varies inversely with the pressure  exerted by the gas if the temperature and number of moles are held constant. The experiment  could have been improved if a better, more precise scale was used because the scales used in the  experiment were older and it was difficult to get an accurate read.  The second part of the experiment involved the Ideal Gas Law and the molecular weight  of gases. This experiment worked because it was successful in accomplishing the purpose which  was to measure the density and molecular weight of a gas using a 60 mL hypodermic syringe.  Using the Ideal Gas Law (PV=nRT), the molecular weight of an unknown gas was determined to be 9.366 g/mol. The rearranged formula used was MW= (mRT)/(PV). Since the molecular  weight of the unknown gas was 9.366 g/mol, it was closest to the molecular weight of CH4,  which is 16.04 g/mol. So, it was hypothesized that the unknown gas was CH4. The experiment  could be improved if the syringe could have been massed without being in a beaker. It is possible that weight of the beaker (used as a holder) interfered with the massing of the syringe with the  gas and nail and caused an error.  Finally, the third part of the experiment involved the relationship between volume and  temperature of a gas. This experiment was effective because it achieved the purpose of  measuring the relationship between volume and temperature. It was found that as temperature  decreased, volume also decreased. It was found that the volume was 142.7 mL at 102.0˚C and  25.6 mL at 21.5˚C. These results were expected because Charles’ Law states that volume of a  gas varies directly with the absolute temperature (K) if pressure and number of moles of gas are  constant. There was error in this experiment though because the percent error between the  calculated volume and the measured experimental volume was 15.0%. Error could have occurred if some water was lost in the transfer between the Erlenmeyer flask and the graduated cylinder.

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