Experiment 1 Molar Gas Constant 1. Objective 1.1. To comprehend the definition of ideal gas 1.2. To master the ideal gas

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Experiment 1 Molar Gas Constant 1 Objective 1 1 To Comprehend The Definition Of Ideal Gas 1 2 To Master The Ideal Gas 1 (119.84 KiB) Viewed 58 times

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 learn 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 4.3. Pour about 5 mL of 6 M HCl into 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 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 V. 4.6. Shake the aluminum into the acid. It will begin to react quickly and produce Ha 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 at 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 V2. The volume of a gas can be obtained from the difference between V2 and V. (V-V-V). 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 po from the pVERT (1-1) where p. V. and T are the pressure, volume, and absolute temperaturen 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 Hz gas. The Ha will be generated using this reaction: 2Al + 6HCI AICI + 3H: 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 H2 produced. By measuring the mass of Al 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 HCI: 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. 4.2. Cut a piece of aluminum foil and weigh 25 mg using an electronic balance. atmospheric pressure (Ps= P.-P. 4.10. Clean up the tube. 5. Data Analysis 5.1. Fill out the table with both the original data and the calculated results. 100g me 10/mol Vix 10m V 10/m Ve 10m TIR po 10 Pa pe 10 Pa P10 Pa 5.4. Determine the molar gas constant using the ideal gas law, and compare literature data with the 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?