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CHEM 103 Lab Report 5 Gas Laws (GRADED A) Latest Update (100% Correct Elaborations)
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- CHEM 103
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- Portage Learning
CHEM 103 Lab Report 5 Gas Laws (GRADED A) Latest Update (100% Correct Elaborations)
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This study source was downloaded by 100000884123152 from CourseHero.com on 04 -13-2024 14:08:43 GMT -05:00 https://www.coursehero.com/file/190382352/Chemistry -Lab-Report-5docx/ CHEM 103 Lab Report 5 Gas Laws (GRADED A) Latest Update (100% Correct Elaborations) Chemistry Lab Report Experiment #: 5 Title: Gas Laws Purpose: The study of gasses, their laws, and how they affect atmospheric pressure. Procedure: We are going to be looking at a tool where we can demonstrate Boyle’s law with a syringe fitted in a base and it is capped off with a wooden base and platform where we are going to place weights. We are going to be looking at pounds per square inch and right now it is about 14.3. If we look at our plunger without any weight on top the atmospheric pressure is about 33 mL (the volume). We are going to demonstrate Charles’s Law with a flask that is in ice. We are going to pull out the flask and note its initial temperature and then attach the syringe. The syringe’s plunger will be down and then we are going to use a hair dryer to keep the temperature up. We will notate the volume every five degrees of temperature change. The volume of the flask is about 328 mL. Initial temperature: 6.5 degrees. The hair dryer then begins warming the flask. We are going to calculate the mole or mass of a substance. n= m/M m. PV= nRT or PV= m/M m(RT) or Mm = mRT/PV. We are going to calculate the molar mass for acetone. We are going to put acetone in a flask, heat the flask up, and then fill the flask with aceton e gas. The opening of the flask is covered with foil and a hole was made with a paperclip to help release oxygen and excess acetone. The weight of the flask and foil is 112.1373. The professor inputs the 1.8 mL of acetone into the flask, clamp the flask, a nd set it in a water bath. Acetone has a boiling point of about 57 degrees. We are going to heat the acetone to about 65 degrees. This ensures the acetone This study source was downloaded by 100000884123152 from CourseHero.com on 04 -13-2024 14:08:43 GMT -05:00 https://www.coursehero.com/file/190382352/Chemistry -Lab-Report-5docx/ is fully vaporized. It takes about 15 minutes for the temperature to raise to about 66 degrees. The temperature is 66.4 °C. Still working with the ideal gas law where we will measure the moles of gas produced from a react ion. The reaction is CaCO 3 (s) + 2HCl (aq) → CaCl 2 (aq) + H2O (l) + CO 2 (g). We are using a gas apparatus to calculate which has a reaction chamber (with a syringe where we will be able to inject into a test tube), a tube, a glass burette, another tube that leads to the leveling bowl. One thing we always need to check for is make sure everything is airtight and to know it is airtight you can move the leveling bowl and see that the water in the burette is lowered. If it is not airtight the liquid in the b urette will move up and down with the leveling bowl. The professor puts 2 mL of HCl in the syringe and 0.2152 g of CaCO 3 in the test tube. We then need to check again and make sure everything is airtight. The starting point of volume of water with green food coloring in the burette is 12.2 mL. Data/Results/Calculations: We are going to add a 2.5-pound weight and the gas that is trapped in there decreases to 27 mL. With a second weight, now 5 pounds, it decreases to 22.5 mL. With three weights, 7.5 pounds, it decreases to 18 mL. With four weights, 10 pounds, it decreases to 16.5 mL. The final weight is added, and it is five pounds, giving us a total of 15 pounds, the pressure then decreases to 13.0 mL. The professor uses the hair dryer to warm the flask for about three minutes and you can see the plunger in the syringe rise as the flask heats up. We have almost reached the maximum volume of the syringe. By 36.5 degrees the plunger raised to about 23.5 mL. That happened because we cooled the glass in the flask to about six degrees and it was open to the atmosphere and the gas expanded to the only place it had to go which was the syringe.The benefits of buying summaries with Stuvia:
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