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graygnat922Lv1

28 Nov 2020

An enclosed tank containing a liquid of density p has a hole in its side at a distance y₁ from the tank's bottom. The hole is open to the atmosphere, and its diameter is much smaller than the diameter of the tank. The air above the liquid is maintained at a pressure P. Determine the speed of the liquid as it leaves the hole when the liquid's level is a distance h above the hole.

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Iris MandiaLv9

17 Jan 2021

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I need help writing a purpose for a chemistry experiment. I feel I was always do a great job, but my professor always disagrees and Iâm out of ideas. The professor wants us to summarize the introduction, and summarize what you will do in each section of the experiment and state how this work will support the goal of this experiment being longer than 1/2 a page. Please, please help me right a better purpose for the experiment below. Thanks.

Experiment 9 Molecular Weight Determination of a Pure Substance Using the Ideal Gas Equation.

Introduction:

The purpose of this experiment is to determine the molecular weight of a volatile, essentially non-polar liquid. An excess amount of pure unknown volatile liquid will be placed into a flask, whose volume will also be determined. The flask will be placed into a hot water bath, whose temperature corresponds to the temperature of the gas in the flask. The liquid will evaporate, driving out the air while the excess liquid evaporates. The pressure of the gas in the flask will correspond to the atmospheric pressure. After the excess unknown liquid has been allowed to evaporate, the flask will be stoppered, cooled, and weighed to determine the grams of the unknown liquid that will be present at the temperature of the water bath as a gas. In this experiment the ideal gas equation will be used PV = nRT = (g/M)RT where R = 0.0821 L*atm/mol*K, T = temperature in K, P = pressure in atm, V = volume in liters, n = moles of gas, g = grams of gas, and M = molecular weight of gas (in units of g/mole). Solving for the molecular weight, M: M = gRT/ PV.

If the molecular weight of a gas is to be determined, the m, T, P, and V must be determined experimentally in the lab. Even though the ideal gas equation is only an approximation of the behavior of gases, molecular weights can still be obtained within 5% of the correct values, as long as volatile non-polar compounds or compounds with only slight amount of polarity are used. For example, C, H, compounds as CH₄ are essentially non-polar, whereas compounds as H₂O are highly polar. Hence, the ideal gas equation would not be a good approximation for describing the behavior of gaseous water.

Procedure:

At the very beginning of the period get a one-liter beaker. Put about 800 mL (your instructor will tell you the exact amount needed) of tap water into the one-liter beaker. Put the one-liter beaker with water onto the hot plate. Set the heat setting of the hot plate to the maximum value. The water in the beaker should be boiling very lightly prior to doing the actual experiment. Therefore, after the water starts boiling in the hot water bath, it may be necessary to cut the heat setting back from highest value. This will take some time. While the water is heating, get the rest of the things needed for this experiment. The setup is shown in figure 1. Record the barometric pressure (in torr to one decimal place). Obtain the rest of the setup consisting of a 250 ml flask, properly prepared rubber stopper with glass tube and aluminum foil, a no-hole rubber stopper, thermometer, and glass stirring rod.

Make sure the 250 mL Florence (or Erlenmeyer) flask is dried (if it is not dry, rinse with 5 mL of acetone, pour off the acetone into the waste bottle in the hood, and then clamp the 250 mL Florence flask onto the ring stand in the inverted position to allow the last traces of acetone to drain out and evaporate. Place the dry no-hole stopper on the flask and weight the flask with the rubber stopper on the balance to 3 decimal places. Record this weight for the weight of the flask plus rubber stopper and moist air. Place 5 mL with a graduated cylinder of unknown liquid into the flask. Place the one-hole rubber stopper, with tube and aluminum foil in the flask. This one-hole stopper, which contains a glass tube that sticks out on the top by 3 mm and is flush with the bottom of the stopper, is covered with aluminum foil with a hole punched into the bottom where the glass tube is. This one-hole rubber stopper is already prepared for you. Push it down firmly into the flask. Remove it. Do this 2-3 times to smooth out the aluminum foil so that the stopper will go down into the flask as much as possible. Then push the stopper down so that it fits snugly but not too tightly to allow it to be removed while the flask is hot. Clamp the flask about the top lip of the Florence flask. That is, the center of the clamp goes about the rim of the flask. Push the flask as far down into the water bath as possible while holding the end of the clamp with your other hand. It is important to be sure that the water in the water bath is always at least 5 mm above there the bottom of the stopper is in the flask. More water may have to be added as some of the water evaporates during the duration of this experiment. (A beaker with hot water (extra) should be present in the hood. One or two of these beakers of hot water should be enough for everyone.) If the water level is not kept to its proper height, the liquid will condense in the upper part of the flask and the excess liquid will never be removed. Be sure that the aluminum foil on top makes a protective wind breaker for the short glass tube sticking out of the rubber stopper so that condensation does not occur there also. As the liquid evaporates from the flask, mix the water in the water bath occasionally and check to see that the temperature remains constant. Record the temperature value of the water bath as the temperature of the gas in the flask for the temperature of the gas would have equilibrated to the temperature of the water bath. After all the liquid has evaporated (takes 2-5 mins for the liquid to evaporate.) from the flask (check carefully that all of the liquid has evaporated-since observing when all the liquid has been evaporated maybe difficult, you should carefully shake slightly the clamp holding the Florence flask to observe the movement of the unknown liquid and when it has disappeared) and none is condensed on the surface walls; (if condensation occurs, be sure all precautions mentioned above are taken) then (these next several steps are to be done quick) remove the rubber stopper with the glass tubing and aluminum foil without excessive shaking. There could be a condensed liquid droplet or two in the glass tube that is not visible. The droplets could drop back into the flask and cause a false high reading for the measured weight of gas in the flask. Immediately replace the rubber stopper (with the glass tube and aluminum foil) with the no-hole stopper, which was used when the flask was originally weighed. This step must be performed quickly to prevent the unknown gas vapors from escaping and being replaced by moist air. Place the no-hole rubber stopper in the Florence flask firmly. Remove the flask from the bath and again check to be sure that the no-hole rubber stopper is firmly in place. Cool the flask by running tap water over the flask for 30-60 seconds. If the stopper is not fitted firmly, air will enter the flask as the liquid inside the flask condenses. As the gas cools and changes to the liquid state, a partial vacuum is created inside the flask. Hence, air will enter the flask if the rubber stopper is not fitted firmly. Completely dry the flask and weigh it on the balance to three decimal places. Record the weight of flask plus stopper and unknown gas.

Repeat this entire procedure a second time and record the date. After, second trial, completely fill the flask with distilled water. Place the no-hole rubber stopper in the flask allowing the excess water to overflow. Wipe the outside completely dry. Then measure the volume of the water in the flask by pouring water into a graduated cylinder. Record this volume.

1. When an open-end manometer is attached to a tank of gas in which the pressure is 1.030 atm which of the following will be observed if the barometric pressure is 0.980 atm? (Conversion factor: 1 atm = 760 torr)

a.The mercury level in the open arm of an open-end manometer will be 19 mm above a reference point.

b.The mercury level in the open arm of an open-end manometer will be 38 mm above a reference point.

c.The mercury level in the arm connected to a tank of gas will be 19 mm above a reference point.

d.The mercury level in the open arm of an open-end manometer will be 38 mm below a reference point.

e.The mercury level in the arm connected to a tank of gas will be 38 mm below a reference point.

2. A 15.0 L bulb containing Ar at 5.0 atm and a 22.0 L bulb containing Kr at 7.0 atm are connected by a stopcock. What will be the partial pressure of Ar in the mixture when the stopcock is opened and gases are allowed to mix at a constant temperature?

a.4.9 atm b.2.0 atm c.5.0 atm d.3.0 atm e.0.41 atm

3. A gaseous mixture contains equal masses of CO2, CO, N2, and O2. If the total pressure of the mixture is 1.00 atm what can be said about partial pressures?

a.Partial pressures of all gases are equal to 0.25 atm.

b.Partial pressure of N2 is smaller than partial pressure of O2.

c.Partial pressure of O2 is greater than partial pressure of CO.

d.Partial pressure of CO is more than 0.25 atm

e.Partial pressure of CO2 is greater than 0.25 atm.

Gas absorption or gas scrubbing is a commonly used method for removing environmentally undesirable species from waste gases in chemical manufacturing and combustion processes. The waste gas is contacted with a liquid solvent in which the potential pollutants are highly soluble and the other species in the waste gas are relatively insoluble. Most of the pollutants go into solution and emerge with the liquid effluent from the scrubber, and the cleaned gas is discharged to the atmosphere. The liquid effluent may be discharged to a waste lagoon or subjected to further treatment to recover the solvent and/or to convert the pollutant to a species that can be released safely to the environment. A waste gas containing SO2 (a precursor of acid rain) and several other species (collectively designated as A) is fed to a scrubbing tower where it contacts a solvent (B) that absorbs SO2. The solvent feed rate to the tower is 1000 L/min. The specific gravity of the solvent is 1.30. Absorption of A and evaporation of B in the scrubber may be neglected. The gas in the scrubber rises through a series of trays (metal plates perforated with many small holes), and the solvent flows over the trays and through down comers to the trays below. Gas bubbles emerge from the holes in each tray and rise through the covering liquid, and SO2 diffuses out of the bubbles and into solution. The volumetric flow rate of the feed gas is determined with an orifice meter with a differential mercury manometer being used to measure the pressure drop across the orifice Calibration data for this meter are tabulated here: The molar density of the feed gas may be determined from the formula where P and T are the absolute pressure and temperature of the gas. An electrochemical detector is used to measure the SO2 concentration in the inlet and outlet gas streams: SO2 in the sampled gas is absorbed in a solution across which a fixed voltage is applied, and the mole fraction of SO2 in the gas is determined from the resulting current. The calibration curve for the analyzer is a straight line on a semi log plot of y(mol SO2/mol total) versus R (analyzer reading), which passes through the following points: The following data are taken:

Refer to charts and flow diagram from this url:
http://www.solutioninn.com/engineering/chemical-engineering/chemical-processes/gas-absorption-or-gas-scrubbing-is-a-commonly-used-method

(b) Determine (I) the orifice meter calibration formula by plotting V versus h on logarithmic axes and (ii) the SO2 analyzer calibration formula.
(c) Calculate (I) the mass fraction of SO2 in the liquid effluent stream and (ii) the rate at which SO2 is removed from the feed gas (kg SO2/min).
(d) The scrubber column trays commonly have diameters on the order of 1ï¿½5 meters and perforation holes on the order of 4ï¿½12 mm in diameter, leading to the formation of many tiny bubbles in the liquid on each tray. Speculate on the advantages of making the bubbles as small aspossible.

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