- Besafe Airtel Lte 12 14 Pm O 86 Molar Gas Constant 2 Experiment 1 Molar Gas Constant 1 Objective 1 1 To Comprehe 1 (38.77 KiB) Viewed 71 times
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.. BeSafe Airtel LTE 12:15 PM . 86% Molar gas constant 43. Pour about Sml. of 6 M HClinto the tube 4.4 Put the aluminum into the tube. Make sure that it won't fall into the acid too easily but that you will be able to shake it loose when you want to 4.5. Put the stopper tightly in place. Move the tunnel down some distance and make sure that the difference in height of the liquid level between the buret and the funnel stay the same. Then regulate the liquid level of rubber tube equals with that of hart and record the mark on the burtas 4.6 Shake the aluminum into the acid. It will begin to react quickly and produce Hz pas 4.7. When all of any reaction stops, wait about five minutes for the apparatus to come to room temperature Measure the water temperature as at this time. 4.8. Adjust the height of the funnel so that the level of water in the boret and the funnel are the same. When the heights are the same, the pas pressure inade the tube is the same as the atmospheric pressure in the mom. Now read the gas volume from the water level in the buret as The volume of Hz gas can be obtained from the difference between V. and V. (-) 49. Measure the atmospheric pressure passing a barometer. The pressure of Hus can he obtained by subtracting the saturated vapor pressure of water from the atmospheric pressure -- 4:10. Clean up the tube. 5. Data Analysis 5. Fill out the table with both the enginal data and the calculated results 101 10 ml TE AP 5.4. Determine the molar gas constant using the ideal gas law, and compare it with the literature data 6. Notes 6.1. The apparatus must be loakproof 6.2. Wear poles at all times during this experiment 7. Exercises 7.1. Why it is necessary thu rond V: after the temperature of apparatus cool to room temperature 7.2. Why don't you need to moure the volume of HCl accurately? 2/2 = III O-
Experiment 1 Molar Gas Constant 1. Objective 1.1. To comprehend the definition of ideal gas. 1.2. To master the ideal gas law. 1.3. To leam the way to measure the molar gas constant. 2. Introduction An ideal gas is a theoretical idea: a gas in which there are no attractive forces between the molecules, and in which the molecules take up no space. Both of these assumptions do not exist in reality. However, when the pressure is fairly low (around atmospheric pressure or less) the molecules are not very close to each other. The intermolecular attractions and molecular size are not very important under these conditions. Under these conditions, a gas will behave nearly ideally. This is true for things we readily identify as gases at room temperature and pressure conditions, like hydrogen, nitrogen, and oxygen. These real gases are said to behave ideally, that is, they obey the ideal gas law PV = nRT where p, V, and I are the pressure, volume, and absolute temperature; n is the number of moles of gas; and R is the ideal gas constant, also called molar gas constant. As long as the pressure is not too high, and the temperature is fairly warm, this law is followed very closely by most real gas. The value of R is determined experimentally by measuring the other variables in the equation, and solving mathematically to get the value of the constant. R is the same for all gases, given the gas has ideal behavior. In this experiment you will determine the molar gas constant using H2 gas. The Hz will be generated using this reaction: 2A1 + 6HCI-2AICH + 3H21 From the balanced equation, you can see that there is a simple ratio between the number of molecules of Al used and the amount of Hz produced. By measuring the mass of AI we can calculate the number of Al produced, and thus determine n for the ideal gas equation. T can be measured with a thermometer, p from a barometer, and V will be measured in a special gas buret. With these four pieces of information, you'll be able to calculate R. 3. Apparatus and Reagent Gas buret apparatus; thermometer, electronic balance; 6 M HCl; aluminum foil. 4. Procedure 4.1. Set up the gas buret apparatus, but leave the stopper out of the tube and bure at this time. Clamp the buret, and the funnel near the top of the ring stand. Fill the buret with water until the level of water is at the mark on the buret, and just at the bottom of the funnel. Then inset the stopper into the top of the buret. Cum foil and waiah 25 mawinlarni halan
4.3. Pour about 5 mL of 6 M HCl into the tabe. 4.4. Put the aluminum into the tube. Make sure that it won't fall into the acid too easily. but that you will be able to shake it loose when you want to 4.5. Put the stopper tightly in place. Move the funnel down some distance and make sure that the difference in height of the liquid level between the buret and the funnel stay the same. Then regulate the liquid level of rubber tube equals with that of buret and record the mark on the buret as Vi. 4.6. Shake the aluminum into the acid. It will begin to react quickly and produce Hz gas. 4.7. When all sign of any reaction stops, wait about five minutes for the apparatus to come to room temperature. Measure the water temperature as Tat this time. 4.8. Adjust the height of the funnel so that the level of water in the buret and the funnel are the same. When the heights are the same, the gas pressure inside the tube is the same as the atmospheric pressure in the room. Now read the gas volume from the water level in the buret as Vs. The volume of H: gas can be obtained from the difference between V2 and V (V, V, -1). 4.9. Measure the atmospheric pressure po using a barometer. The pressure of Hz gas can be obtained by subtracting the saturated vapor pressure of water p* 1,0 from the atmospheric pressure ( PH, = P.-P'1,0). 4.10. Clean up the tube 5. Data Analysis 5.1. Fill out the table with both the original data and the calculated results. A 10% me x 10 /mol Vi 10m Vix 10m Pie x 10m TIK po 10-P pox 10 Pa Pre> 10%P. 5.4. Determine the molar gas constant using the ideal gas law, and compare it with the literature data 6. Notes 6.1. The apparatus must be leakproof. 6.2. Wear goggles at all times during this experiment. 7. Exercises 7.1. Why it is necessary that read V after the temperature of apparatus cool to room temperature? 7.2. Why don't you need to measure the volume of HCl accurately?