Share. V��h,F����U�o�R�O����4�f:Dq6����嫦oB-�K ����ɛ���4AA A laboratory group measures an excess of an unknown liquid. Topics In Chemistry (SCC 101) Academic year. For our experimental conditions today, we can assume that hydrogen gas adheres to the ideal gas law. 1. Materials Ideal Gas Law Lab 1. When the temperature and pressure remain constant. Y�Q�,�X�(?�gS4 504 0 obj<>stream Adjust the height of the funnel so that the level of water in the funnel is at the same height as the level of water in the burette. The reading is 74.8 cm when true atmospheric pressure is 76 cm and temperature is 30 They heat the sample n a water bath until all liquid has been vaporized for several minutes. You may have to adjust the height of the funnel relative to the rest of the apparatus. Be careful not to allow any of the HCl to flow through the rubber tubing connecting the large test tube and the burette.
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474 31 Finally determine the percent purity of the zinc sample by dividing the mass of zinc reacted by the mass of the impure sample and multiplying by 100%. 0000006395 00000 n Also, complete this “Ideal Gas Law Pre-Lab Activity” to hand in at the beginning of class on Friday, September 27th. Use a graduated cylinder to fill the flask with water. Since the attractive forces between molecules do exist in real gases, the pressure of real gases is actually lower than of the ideal gas equation. It involves the measurement of the volume of hydrogen gas generated from a reaction of zinc with excess hydrochloric acid. To determine the pressure of hydrogen gas alone, you will need to use Dalton’s Law of Partial Pressures. stream Vapor pressure of water (PW) from Table 1, Observations: Use the numbered steps from your procedure followed by your observations. Please sign in or register to post comments. Explain.
To obtain the vapor pressure of water at a given temperature, refer to Table 1 in page 2. How? DOCX, PDF, TXT or read online from Scribd. L�1Ks=�н�;%nB�2l�6u��h���$/��O)��W���w����S��� h�_� The ideal gas has constant, random and straight-line motion. ��'��. The student responsible for lowering the funnel must do so, when necessary, after the HCl and zinc have been mixed so that the level of water in the funnel is at the same height as the level of water in the burette. Pressure is inversely proportional to Volume, Volume(V) is directly proportional to the Amount of gas(n), A ballon with 4.00g of Helium gas has a volume of 500mL. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. While the flask is cooling, obtain the pressure of the laboratory from the barometer at the front of the room. Write out the balanced chemical equation for the reaction you will perform today (including phase labels.) Pre-Lab Questions *Note – This pre-lab must be completed before you come to lab. w�A�v�~l�ґ���ܱ��6K{�oU�l�q�ZA�ct_�/ݮ4����.��cP����:�wI��)�H������=�ء���G��~\�j��z����2�YLb�.{����`3\�����(���^:���]�{��J�(��H=��I,�9[��ق? Feedback . Discover everything Scribd has to offer, including books and audiobooks from major publishers. A short clip to show how to set up the LabQuest for the Gas Laws lab.
Give the units for each variable.
PH2 = partial pressure of hydrogen gas = PA- PW. Otherwise the key variables are: Since we need to solve for the final temperature you can rearrange Charles's: Once you plug in the numbers, you get: T2=(308.15 K x .75 L)/(1.25 L) = 184.89 K. Using Avogadro's Law to solve this problem, you can switch the equation into \( V_2=\frac{n_1\centerdot V_2}{n_2} \). This condition is considered in the van der waals equation. 0000006084 00000 n temperature times the gas constant, PV = nRT. H�TP=o� ��+��-��&�I�@����^����g?���K�l���1��NG���G�q�V�ը&�dq�� ��mې�L�)�p7�z�5j�֍9s��9�/!|�.! EXPERIMENT 6: USING THE IDEAL GAS LAW TO DETERMINE PURITY OF A ZINC SAMPLE, Lansing Community College General Chemistry Laboratory I, DATS SHEET FOR EXPERIMENT 6 - USING THE IDEAL GAS LAW TO DETERMINE PURITY OF A ZINC SAMPLE, POST LABORATORY FOR EXPERIMENT 6 - USING THE IDEAL GAS LAW TO DETERMINE PURITY OF A ZINC SAMPLE. 0% found this document useful, Mark this document as useful, 0% found this document not useful, Mark this document as not useful, Save Gas Laws Prelab Questions for Chemistry I For Later. %PDF-1.4 %���� The reaction between 6.0 M HCl and zinc occurs rapidly after mixing. Pour all the contents of the large test tube into the labeled zinc chloride waste container in the hood. H��SɊ�0��)�� cE�w9$J�"zIK�����K����To�Z����O�&��<2��y����������j����Y0�� +l�qB��W�!��X��7�9 �ƘTX^`�i�Hh����.ޕmm�A�'�`�6��M�`O�����adֹ�~��9��w�ӛ��SM�ÆදF{:�@�k�L�4�;�i�e.xo^�r/rT�\�J((d[{���s J�A�Bj��, 0000008029 00000 n What type of suggestion do you have? "Properties Relative to Ideal Gases. Calculate the mol of gas in the flask using the ideal gas law: b. Today’s experiment is an example of a single replacement reaction. Turn the heat source off. Legal. Measure the temperature of the water in the funnel using a thermometer. (2 pts.
0000004686 00000 n Gram of Zn reacted = _____ mol H2 x = _____ g Zn Equation 6. The LibreTexts libraries are Powered by MindTouch® and are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. Obtain the mass of the flask, foil and rubber band. Legal. Record the mass of the zinc in your DATA TABLE. 0000005569 00000 n An ideal gas follows the ideal gas law at all conditions of P and T. The particles in an ideal gas do not have finite size and volume. Mass of flask, foil, wire, and volatile liquid AFTER heating, Volume of flask (if more than one graduated cylinder of water added, add the volumes to obtain the final). \[ n_1 = \frac{4.00g}{4.00g/mol} = \text{1 mol} \], \[ =\frac{2 mol \centerdot 500mL}{1 mol}\]. �Dc$H��R��ل-.� 0�5c��9���%'�"?8i{��O����m�JU ;� n�c������-$��S����. %PDF-1.3 Fill a 600 mL beaker with water and add a few boiling stones. For each run use a clean, dry set of glass tubes from the side bench. University. Connect the large test tube to the apparatus while keeping the small test tube containing the HCl in the vertical position. Experiment 2: Charles' Law. They add this to an empty flask for which they calculate the volume. b. Charles' law: Volume divided by Temperature equals constant # of moles times gas. Place the large test tubes in the tray and the small test tubes in a 400 mL beaker found next to the oven. Hydrogen gas generated in today’s experiment is, however, a real gas not an ideal gas. The small test tube should be in the vertical position (mouth pointing upwards). LAB Report 10 - Determination of the Gas Law Constant. mol-1. 0000003938 00000 n We'd love to have your feedback Which subject best describes your feedback? Once the reaction has subsided, gently incline the test tube again so that more HCl comes in contact with the zinc. Use the average deviation value to discuss precision. Record the volume of water in the burette to the nearest 0.01 mL as your initial burette reading in the DATA TABLE. 0000009367 00000 n Remove the flask from the water and allow the flask to cool. Have questions or comments? x�b```b``mf`2�02 � P������D���|�c���Jw蘈g00LI����0�q�0y�4\O��*�x�aR�I��ʣ7R�q>���̠���ӢL�>��y�M���&�|V�˔��HI�WRȠ��9&�I��ݴL2#��a�t��;:�ֈ���B*�P���� endstream endobj 475 0 obj<>/Metadata 40 0 R/PieceInfo<>>>/Pages 39 0 R/PageLayout/OneColumn/OCProperties<>/StructTreeRoot 42 0 R/Type/Catalog/LastModified(D:20070315105314)/PageLabels 37 0 R>> endobj 476 0 obj<>/PageElement<>>>/Name(HeaderFooter)/Type/OCG>> endobj 477 0 obj<>/Font<>/ProcSet[/PDF/Text]/Properties<>/ExtGState<>>>/Type/Page>> endobj 478 0 obj<> endobj 479 0 obj<> endobj 480 0 obj<> endobj 481 0 obj[/ICCBased 499 0 R] endobj 482 0 obj<> endobj 483 0 obj<> endobj 484 0 obj<> endobj 485 0 obj<> endobj 486 0 obj<> endobj 487 0 obj<>stream If any of the HCl comes in contact with the zinc, you will have to start the experiment all over again. PT = atmospheric pressure provided by your instructor, PW = vapor pressure of water at temperature T. The grams of zinc present in the impure sample can be determined by using the calculated the moles from equation 4. 0000014044 00000 n Be very careful during this process so that water does not flow through the rubber tubing used to connect the large test tube to the burette. 1. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. 0000000016 00000 n H��T�n�0}�+�#H��LU�&��N�V���}����Q��Y�~��M�&]�)Jb��{�%:�M�$+��ѹ1�Z��Ge��cTn:ѭ��Z���M&��SΈH Kb��҄�4N!K)��xv6���}�Bt3�0�w����Pi�A��Wx>�I�EeI�A��QBie�w�+{{9 ������!�d+��)Ar�w�3?2�A�X~�.K�������j��^_`�W�BK�&��Xl�0�Cu+.2"d4%̡���N�����?w�{��CDj�F��c��dq����(˅�+9�W����cx��)�"�`����ƇuٛwTX1�2���H1/b��Z���-+�z��r�of)�$˭�3|�5�E=�Zヮ�A��no�%�ꦁ����L��˵V�Z(�P=L�M�8�C���i ����ۚ䘕Ё���t~r�B�ͲW�>�\j@4Y�&���M�l�Q�U��� d� ��;�� l�=��'����$��m��:�M The sample is cooled and measured.
1. if you weighed 0.50 g of an unknown metal and reacted it with acid as in this experiment to get 188.33 mL of hydrogen gas with an atmospheric pressure of 759 torr and a temperature of 20.2 deg C, what is the atomic mass of the unknown divalent metal and what is the metal? Pre lab for Gas laws? What type of suggestion do you have? Comments. Leave the wet test tubes in a tray next to the oven. Set up the ring stand, ring, tripod and hot plate as shown in the diagram. The hydrogen gas produced will be collected over water in a buret. Only once the flask has cooled, obtain the mass of the flask set-up and record your data. The pressure remained constant and since the amount of gas is not mentioned, we assume it remains constant. 2. 4 0 obj H�tT]o�0|ϯ��Dj�����>�V�V��I䭭N� Pour the contents of the large test tube into a labeled waste container in the hood. 2.
Use your data to calculate the percent purity of zinc. Water temperature = 22.1 degrees Celsius Barometic Pressure = 763.9 mm Hg Volume of air (before) = 30mL Volume of air (after) = 68mL Rate of change = 38mL 2. Boyle's law: Pressure times Volume equals constant # of moles times constant. Top. After the final trial remove the cover assembly and rinse the flask thoroughly. You will use the ideal gas law to determine the moles of hydrogen gas generated in this experiment. To solve this question you need to use Boyle's Law: Keeping the key variables in mind, temperature and the amount of gas is constant and therefore can be put aside, the only ones necessary are: Plugging these values into the equation you get: To solve this question you need to use Charles's Law: Once again keep the key variables in mind.