CHEMISTRY (CHEM 103) LAB REPORT 5 | PORTAGE LEARNING|WITH PROCEDURES, EXPLANATION AND FINAL RESULTS/ VERIFIE D/LATEST UPDATE 2024 -2025 Chemistry Lab Report Experiment # 5 Title: Purpose: To understand gas laws and see how they work through multiple experiments. Procedure: Boyle’s Law: P= k/ V P₁ X V₁= P₂ X V₂ Pressure units pounds (lbs) per square (in²) Pressure in lab: 14.3 psi Area of syringe plunger head: .75 in² Pressure of a gas is inversely related to its volume As pressure and volume change High pressure/ Low volume Pressure goes down/ increase volume weights on plunger 1. Place plunger with atmospheric pressure is 33 mL; with weight of 2.5 lbs, the volume is now 27 mL and the gas is getting compressed as plunger pushes it down. With 2x2.5 lbs a total of 5 lbs, with volume of 22.5 mL, 2x2.5 a total of 7.5 lbs 18 mL, with 10lbs of weight is 16.5 mL of volume, a total of 15 lbs is 13 mL of volume. The higher the pressure, the smaller the volume. Charles Law: Volume and Temperature are related V= K * T As we increase volume the temp will increase As we increase temp the volume increase V₁/T₁ =V₂/V₂ Intial temperature 6.5 °C/ Initial Volume : 328 mL Final Temperature 36.5°C, th eplunger was raised to 23.5 ml (total of 315.5 mL) 1. The Flask has been cooling and has a syringe and thermometer. Attach a syringe to the flask. Place the thermometer to measure the volume of the beaker. Measure initial temp and volume using the 328 ml flask. As volume or temperature increases the other will increase as well. Use a hair dryer to warm up the flask. Every 5 degrees increase, record temp and volume of syringe. The plunger should be raised with temperature increase. As the gas expands it will go up into the plunger. Ideal Gas Law 1: PV=nRT, V=nRT/P V= (1.0 mole X 0.0826 L-atm/mol - k x 273K) / 1.0 atm=22.4L n=m/M ◻(molar mass) M◻=mRT/PV STP (Standard Temperature and Pressue) : 0.0 °C (273 K) at 1 atm pressure -Atompsheric pressure is premeasured:0.9766 atm -Volume of flask is premeasured : 328 mL 1) Get the flask and put foil and put foil on the opening of the flask, use a paperclip to place a small hole in foil for excess oxygen and acetone to exit. Place flask with foil on scale andmeasure mass : 112.1373. Fill the flask with 1.8 mL of acetone. Clamp the flask, and set in the water bath m, turn the flame on . Heat until 65 °C to ensure the acetone is vaporized and fills the flask. Heat for 13 min later and check back . Continue to wait until 66 °C and turn off the flame when it hits 66 °CCalculate temperature beforetaking flask out to 66.4 °C. Take the flask out and place it in cool water. Wait for a couple of seconds to recondence acetone back to liquid. Unclano the flask and dry off any water from it. Place the flask with foil back on scale and c alculate new mass : 112.7900, Calculate molar mass. Ideal Gas Law 2: Measuring Moles of Mass produced from a reaction CaCO3(s) = 2HCI (aq) -> CaCI2 (ag) + H2O (I) + CO2(g) Pv=nRT -Mass of calcium carbonate : 0.215g -Room Temperature is 22.5 °C -Pressure atmospheric temperature 0.9766 atm
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