temperature‚ volume‚ and pressure. Objectives: Conduct a set of experiments‚ each of which illustrates a gas law. Gather data to identify the gas law described by each activity. Complete the calculations necessary to evaluate the gas law in each activity. From your results‚ derive a single mathematical relationship that relates pressure‚ volume‚ and temperature. Hypothesis: As the temperature increases the pressure increases and if temperature decreases the pressure decreases. Also as the volume
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rules to help us do the experiment. We will investigate three properties of gases pressure‚ temperature‚ and volume. By doing this experiment we will be able to define the gas laws. According to Boyles‚ it states that a fixed amount of ideal gas that is kept at a fixed temperature‚ that the pressure and volume are inversely proportional‚ if the temperature stays unchanged. According to Charless Law‚ if the pressure of a gas is held constant‚ as the gas is heated‚ its volume will increase and that
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Absorption…………………………………………………..... 13 Spreading Loss………………………………………………..14 Range‚ SNR…………………………………………………....14 Multipath………………………………………………………16 Communication in underwater acoustic sensor networks Introduction…………………………………………………..18 Need for acoustic sensor networks…………………………..18 Drawbacks in the existing access control And routing protocols………………………………………..19 UW-ASN communication architecture……………………….21 A protocol
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Measurements of temperature change are taken with microLAB sensor and graphed using microLAB software. A final determination of experiments determined absolute zero versus actual absolute zero will be calculated to determine percentage of error in experiments data using Charles’ quantitative law of V1/T1=V2/T2. Obtain a reference of pressures effects on gas using Boyle’s law using a gas sample of standard “air” within a syringe and measuring pressures increase and decrease in association to changing volume
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CaCO3 Kim Wipes 1 M HCl (aq) Mg Ribbon Quantitative balance Pressure sensor GLX Machine Syringe with white connectors Tygon Tubing 125 mL flask with one-hole stopper 50 mL graduated cylinders Procedure Record the Temperature and convert into K Determine the volume of the Flask and Tygon Tubing you will be using Connect the Pressure sensor to the GLX Machine and then connect the Tygon Tubing to the Pressure Sensor. Weigh the Mass of the Mg Ribbon and The CaCo3 and wrap it into a
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Introduction to Design of Industrial Ventilation Systems Course No: D02-001 Credit: 2 PDH J. Paul Guyer‚ P.E.‚ R.A.‚ Fellow ASCE‚ Fellow AEI Continuing Education and Development‚ Inc. 9 Greyridge Farm Court Stony Point‚ NY 10980 P: (877) 322-5800 F: (877) 322-4774 info@cedengineering.com An Introduction to Design of Industrial Ventilation Systems Guyer Partners 44240 Clubhouse Drive El Macero‚ CA 95618 (530)7758-6637 jpguyer@pacbell.net J. Paul Guyer‚ P.E.‚ R.A. Paul Guyer
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produced in various reactions. The Ideal Gas Law was needed in order to calculate the mass of reactants and moles of gas produced: ‚ where is the pressure in atm‚ is the volume in Liters‚ is the number of moles‚ is the ideal gas constant [0.082 (Latm)/(Kmol)]‚ and is the temperature in Kelvins. Considering the units on R‚ it was important to convert pressure‚ volume‚ and temperature to atm‚ L‚ and K‚ respectively. In this investigation‚ the volume of reaction space needed to be measured. One way to
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moles of gas produced. Where P is the pressure in atm‚ V is the volume in Liters‚ n is the number of moles‚ R is the constant 0.0821(atm*L/K*mok)‚ and T is the temperature in Kelvins. In this lab the volume of reaction space needs to be measured. I have chosen to use Magnesium and the amount of H2 gas that the amount of magnesium‚ (.04g)‚ used is 0.00229 mol H2. Procedure 1. Fill a 125 mL flask with 50 mL of HCl (aq) 2. Obtain and set up the pressure sensor 3. Record intial temperature‚( room
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the Boyle’s law (pressure-volume law) indicates that the volume of a certain amount of gas given held at a constant temperature differentiates inversely with the applied pressure when there are constant temperature and mass. Equations: PV=C. When pressure goes up‚ volume goes down (derived from the equation above): P1V1 = P2V2 = P3V3. Furthermore‚ this particular equation dictates that the product of the initial volume and pressure is equal to the product of the volume and pressure after a change under
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Variable- Independent- Amount of Catalase (Filter Paper) Dependent- Amount of Oxygen (kPa) Constant- Temperature in Fahrenheit‚ 2 Pipette of Hydrogen Peroxide‚ 0.8 Cm Filter Paper Punches Materials: * 6 Test Tubes * Vernier Gas Pressure * Sensor * Catalase * Filter Paper Punches * Beaker * Control Group * Test Subject * Safety Goggles * Dropper Pipette * Go Link Procedure- 1. Gather Your Materials Figure 2 2. Put on your goggles
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