gas laws pre lab

Record the final burette reading in your DATA TABLE.

If any part of this is unclear, please consult your instructor. MgCl2!+ H2 The hydrogen gas is the product that is of interest to you in this experiment. Course. H�TP=o� ��+��-��&�΁I�@����^����g?���K�l���1��NG���G�q�V�ը&�dq�� ��mې�L�)�p7�z�5j�֍9s��9�/!|�.! Pour the contents of the large test tube into a labeled waste container in the hood. 4 0 obj Legal. Unless otherwise noted, LibreTexts content is licensed by CC BY-NC-SA 3.0. 1. \[ n_1 = \frac{4.00g}{4.00g/mol} = \text{1 mol} \], \[ =\frac{2 mol \centerdot 500mL}{1 mol}\]. endstream endobj 494 0 obj<>stream endstream endobj 493 0 obj<>stream 0000003396 00000 n When the liquid in the flask has evaporated, you can move to the next step. 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. At this point you should not observe any unreacted zinc. Use your data to calculate the percent purity of zinc. What were some sources of error in your experiment and how did they affect your measurements? In accordance with Dalton's Law, the atmospheric pressure (PT) is equal to the sum of the pressures of hydrogen gas (PH) and the vapor pressure of water (PW): PT = PH + PW                                                                                                                                                                                                                                                                                                                                                                                     Equation 2. �(�#J*��P����FAA O �0�5`0H�XD����Fp�?����`b�MX�آ��P�ƴ�6���\s��^gLah�g�!�������2��)�5�8`a���$�� dk V``�r��x�i20�1�D� ]a ", Ghare, Shakuntala. (It is important that no air bubbles remain in the tubing or funnel stem at the beginning of the 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.

��e��i x/�=�8���v�9�G(X%��\z��E��F��[���Uʍ����&e) �\���7�y�Z.�����a�+,4eq6� K�m5W%^V�Z�.�E�"��P�!D&D��[UKSQ�jse�J�l3#��;�~�%�����U+ �o. 0000001354 00000 n They add this to an empty flask for which they calculate the volume. Pre-Lab Questions *Note – This pre-lab must be completed before you come to lab.

Turn the heat source off. Wipe the outside of the flask to completely remove water being especially careful about drying the top edges. Register now! Record the mass of the zinc in your DATA TABLE. b. Charles' law: Volume divided by Temperature equals constant # of moles times gas. Obtain the mass of the flask, foil and rubber band.

Once the reaction has subsided, gently incline the test tube again so that more HCl comes in contact with the zinc. Vapor pressure of water (PW) from Table 1, Observations: Use the numbered steps from your procedure followed by your observations. 100.0 + 100.0 + 75.6 mL = 275.6 m L     .

PH2 = partial pressure of hydrogen gas = PA- PW. To determine the pressure of hydrogen gas alone, you will need to use Dalton’s Law of Partial Pressures. Zn(s) + 2HCl(aq)  → ZnCl2(aq) + H2(g)                                                                                                                                  Equation 1.

Top. Experiment 3: Gay-Lussac's Law.

Give the units for each variable.

�n�R+��[�@�K|�Ep�p�����ݷ���f��oKL���\쑏�:�yL��.�Ox�缳�+�5:�hޢ�rc�uy�®n@�N��-�}�ZY�Ջ4p�i6�̜�3�}��B��j��T#�k�� U��Q���C�wo���,;VF9O@��r'{�e �0%� c�2�:�ƨ0!e8a���ƒ�5.,_�aN��Mɫ�S���9�՗e����lڡ:AFѧ��ӥZ� vfނ�2�#k2�֦@g=������gM��H�Ob�CL�����b��#�6�"k�)�Yr�Hb3� �5��&��r�[�%��u`u�+�:� ŒԮ�~���Rp���V�hT)�������p��Q�C>؜���.���۸��7��3��2�m>�S�n����!Cd?gϑ5q�K�7h3HfcɁ�8:6r��*�g�s�G��J��P�tS�F?��(���‹���Ï�����ш�T�O���^0��ې�� �} Explain. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. DOCX, PDF, TXT or read online from Scribd. Discover everything Scribd has to offer, including books and audiobooks from major publishers. known amount of gas (H2) at a measured temperature and pressure.

A gas will act like an ideal gas if its gas molecules are small, when the pressure is low, and the temperature is high. 0000009367 00000 n In the space below, write out the ideal gas law (mathematical equation/formula). 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? We'd love to have your feedback Which subject best describes your feedback? You will use the ideal gas law to determine the moles of hydrogen gas generated in this experiment. LaGuardia Community College. Do a complete set of calculations on the data from run 1. 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. %PDF-1.3 They add this to an empty flask for which they calculate the volume. Lab Partner Name: ______________________________.

The collisions between the ideal gas particles are said to be elastic, they exert no attractive or repulsive forces. Y�Q�,�X�(?�gS4 By setting all three laws directly or inversely proportional to Volume, you get: \[ V \propto \dfrac{nT}{P}\] Next replacing the directly proportional to sign with a constant(R) you get: \[ V = \dfrac{RnT}{P}\] And finally get the equation: \[ PV = nRT \] where P= the absolute pressure of ideal gas.

0000011374 00000 n Topics In Chemistry (SCC 101) Academic year. Share. << /Length 5 0 R /Filter /FlateDecode >> If you are not sure about what you should do, please consult your instructor before you proceed to the next step. endstream endobj 503 0 obj<>/Size 474/Type/XRef>>stream 0000005951 00000 n Using a forceps, gently slide the small test tube and contents into the larger test tube containing the zinc powder.

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