Experiment 1: Pressure, Temperature, and Velocity Measurement Objective: The objective of this experiment is to determine the pressure and density of laboratory air, calibrate a pressure transducer and scannivalve, then determine the test section speed as a function of fan speed using three methods of velocity measurement. Equipment: Absolute pressure transducer, digital thermometer, pressure transducer (voltmeter), micromanometer, scannivalve, Pitot tube, low-speed wind tunnel. Part 1: Measurement of Atmospheric Pressure and Density 1. Read the barometer and wind-tunnel thermocouple. 2.
Notice: Look at the DESCRIPTION pane. What is the mass of the lid? How much pressure does the lid exert on the gas? 3. Collect data: With the temperature
Finally, we analyze the errors in both parts of the lab by propagation by substitution and compare the theoretical-experimental values using errors. III. Results: The theoretical buoyant forces for the sphere, the small cylinder, the block, and the big cylinder are 0.297N, 0.131N, 0.369N, and
Materials and Methods 1. Dependent variable. minute ventilation, arterial partial pressure of oxygen and carbon dioxide and pH 2. Independent variable. inhaled gas mixture 3.
Simple and Fractional Distillation of Cyclohexane and Toluene Purpose: The purpose of this experiment was to become familiar with the processes of simple and fractional distillation. In this experiment a mixture of two volatile compounds, cyclohexane and toluene, were separated with the process of distillation. Distillation relies on each compound having distinct and separate boiling points. The pure products were analyzed with gas chromatography to determine the success of the distillation. Introduction: Distillation is the process of heating a liquid until it boils, then condensing and collecting the resulting hot vapors.
2. Explain what relationship exists between the pressure and volume of a gas (assuming a constant temperature), based on your collected data. Answer: The relationship between Pressure and Volume is inversely proportional. As one decrease, the other increases. P1V1=P2V2 3.
Calculations involving the Mole, Avogadro’s Number, Molar Mass, Mole-Mole and Mass-Mole calculations in chemical equations. Combustion analysis and calculation of empirical and molecular formulas from composition analysis. Electrolytes and non-electrolytes. Precipitation reactions and solubility rules. Writing balanced molecular equations and net ionic equations.
LabQuest 34 Vapor Pressure and Heat of Vaporization Vapor pressure or scientifically called equilibrium vapor pressure is the condition wherein the vapor from a liquid over the same liquid in a sealed container is at a point wherein the amount of gas leaving the liquid equals the amount of gas re-entering the liquid from the vapor above the liquid. However there is a mathematical between temperature and vapor pressure, and the Clausius-Clayperon equation attest to this relationship. Clausius-Clayperon equation - ln P = - [∆Hvap / R][1/T] +C The intent of this experiment was to determine the temperature/vapor pressure relationship using the volatile liquid ethanol, CH3CH2OH; and calculate its heat of vaporization. This data was collected over a range of temperatures, 22.4° C to 34.9° C. It was intentional that the temperature remained under 40° C less the pressure inside the Erlenmeyer flask got high enough to pop the stopper out of the Erlenmeyer flask. Materials and equipment: MATERIALS Labquest 20 mL syringe Labquest App two 125 mL Erlenmeyer flasks Vernier Gas Pressure Sensor ethanol, CH3CH2OH Temperature Probe 400 mL beaker rubber stopper assembly 1 liter beaker plastic tubing with two connectors hot plate Procedure: The apparatus was set up as requested by the Lab quest 34 handout and an initial pressure reading of 101.6kpa was obtained at room temperature, 22.4° C. Then the Erlenmeyer flask and the sensors were conditioned to the water bath by holding the flask down into the water bath to the bottom of the white stopper for 30 seconds, and then the valve on the white stopper was closed to keep the ethanol vapor from leaving the container at any time during the experiment.
This will help determine the types of ions present in the water sample. Ions also absorb light differently according to the concentration of the ions in the solution. Using absorption spectroscopy the absorption rate is used to determine which ions are present in the solution and at what concentration. The equation m1v1=m2v2 will be need where m1 and v1 are the initial concentration and volume, and m2 and v2 and the final concentration and volume. Experimental: List of Chemicals 0.5 M NaCl solution 0.5 M LiCl solution 0.5 M KCl solution 0.5 M CaCl2 solution 0.5 M SrCl2 solution Fe/Cu solution containing 400 ppm Cu2+ and 20 ppm Fe3+ in SCN- solution 20 M iron(III) nitrate solution
Introduction: In this lab there were several purposes. Each purpose was to help further the class’s understanding of thermodynamics. Thermodynamics studies the changes in chemical and physical reactions and how energy influences those changes. The purposes of the lab were to decided which of the four given substances would make a good hot pack or cold back, to be able to design a hot pack and cold pack for specified temperature changes, to calculate the amount of heat released or absorbed by one gram of calcium chloride or ammonium nitrate, and to calculate the percentage error in the experiment. In order to understand the lab one must also understand endothermic and exothermic reactions.