MODULE 2 WORKSHEET 6 CALCULATIONS INVOLVING GASES Syllabus reference 9.3.2 1 Two identical gas flasks‚ A and B‚ are kept at the same temperature and pressure. Flask A contains 10 g of ethane gas‚ C2H6. Flask B contains sulfur dioxide gas‚ SO2. Calculate the mass of sulfur dioxide gas in flask B. moles ethane 10/30 0.33 mol moles SO2 0.33 mol mass SO2 0.33 64 21 g 2 What mass of nitric oxide‚ NO‚ is present in a 2.5 L flask at a pressure of 100 kPa and 0ºC? mole NO 2.5/22.71
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Class average for a 80 and 120 drop count was recorded to be 0.041+/- 0.005 mL/drop. If a graduated cylinder is not available there is another way of adding more of the solution. The disposable pipet can transfer 0.5mL of the solution to the chemical reaction. When comparing a 10mL graduated cylinder‚ a 100mL beaker‚ and a 50mL graduated cylinder‚ the most precision peace of glass wear would be the 10 mL graduated cylinder with the true volume of water (calculated)‚ class average‚ and uncertainties
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06.03 Calorimetry: Lab Report Before You Begin: You may either copy and paste this document into a word processing program of your choice or print this page. Instructions: This is a two-part lab. Be sure to follow all steps given in the lab and complete all sections of the lab report before submitting to your instructor. Procedure: Part I: Determining the Specific Heat of a Known Metal 1. Place a plastic measuring trough on top of the digital balance‚ and press the "tare/on" button so that
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Introduction The first law of thermodynamics states that the energy of the universe is constant. Heat is transferred when the atoms of one material vibrate and collide with the atoms of another material‚ thus transferring energy. For this reason‚ heats always travel from hot to cold objects and two objects will reach an equilibrium temperature. Materials and Methods 1. Oven 7. Test Tube 2. Pasco Temperature Probe 8. Stopper 3. Scale 9. Calorimeter 4. Samples of Metals
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Post lab The unknown solution 4055 was tested by the separation scheme in order to identify the four cations that exist in it. The cations found were Ag+‚ Ba2+‚ Mn2+‚ and Ni2+. When I added 5 drops of 3M NaCl to the unknown solution‚ we had some precipitate‚ we centrifuge and then we divided to two test tubes‚ and they were put in hot water and got confirmatory tested. The Ag+ appeared to be in the solution because it melted‚ however Pb2+ didn’t. With the rest of the solution we added Na2SO4 we had
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1 Weigh the beaker. 2 Add 50 milliliters of the solution you want to test to the beaker and record its mass. The mass of the solution is equal to the total mass minus the mass of the beaker. 3 Divide the mass of the solution by its volume -- in this case‚ 50 milliliters -- to find its density. 4 Empty‚ rinse and dry the beaker. Add 4.3 grams of sugar to the empty beaker‚ then add water until the contents reach 50 milliliters in volume. Stir until the sugar dissolves‚ then measure the
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1. The final yield of the cells can be determined by use of an automated cell counter or by use of a hemocytometer (Neubauer chamber). In our laboratory‚ we determine the number of purified cells in a Neubauer-improved‚ bright line chamber with V-slash with a depth of 0.1 mm and a counting area of 0.0025 mm2 from Marienfeld (Lauda Königshofen‚ Germany‚ PN # 0650030). 2. For determination of the final cell yield‚ mix a 10 µl aliquot of the purified cells (Figure 9D) with 10 µl of trypan blue solution
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Name of the Student:………………… Date:………….. What is the volume of 1 mole of hydrogen gas? One mole of any gas occupies the same volume when measured under the same conditions of temperature and pressure. In this experiment you will calculate the volume of 1 mole of hydrogen at room temperature and pressure. Intended lesson outcomes By the end of this practical you should be able to: • further develop skills in manipulating apparatus and accurate measurement; • use the mole concept; • calculate
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Approximately 40 mL of the ionized water was added to the 100 mL beaker‚ then in a 10-mL graduated cylinder‚ 5-mL of HCl was measured then added to the 100-mL beaker of water. The 100 mL beaker was then placed on the assembled ring stand. Approximately 40 mL of the 0.1M NaOH was added to the 250 mL beaker. The 40-mL of NaOH was then added to the buret which was then attached to the ring stand. The LabQuest and the Vernier pH sensor was then hooked up and turned on to measure and graph the pH of the
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Introduction: Discovered in the early 1500s by an alchemist by the name of Paracelsus‚ then observed and recorded by Robert Boyle and later Henry Cavendish‚ hydrogen is the most abundant element on earth and is an essential element for life. This element makes up about 90% of all atoms‚ the most popular being water. Today‚ it is seen as the clean fuel of the future‚ is used in products such as fertilizer‚ and it helps aid in the production of plastics‚ pharmaceuticals‚ and even margarine. Also
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