To derive from experiment the relationships between Pressure (P), Volume (V), Temperature (T), and Water Solubility of gases.

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1 PROPERTIES OF GASES: PRESSURE, VOLUME, TEMPERATURE, & SOLUBILITY RELATIONSHIPS PURPOSE: To derive from experiment the relationships between Pressure (P), Volume (V), Temperature (T), and Water Solubility of gases. VOLUME, PRESSURE, AND TEMPERATURE: Volume, the amount of space taken up by a substance, is described for liquids by the metric units of liters (L), and milliliters (ml), and for solids by the units of cubic centimeters (cm 3 ). The common units of our culture, pints (pts), quarts (pts), and gallons (gal), are rarely used in science. Pressure, the amount of force on an object (or the quantity of collisions with a surface), is measured in atmospheres (atm), millimeters of mercury (mmhg), and Torr. Pressure is measured using a barometer in which a pool of liquid mercury (Hg) is pushed up into a glass vacuum tube by the force of the earth s atmosphere pushing down on it. The height of the mercury in the column is measured in millimeters (mm). One atmosphere of pressure causes the mercury to rise in the vacuum tube to a height of 760 mm or 760 torr (1 atm = 760 mmhg = 760 torr). The culturally common unit of pressure, pounds per square inch (psi) is uncommon in educational science. We will vary the laboratory pressure using either vacuum lines on the bench tops, or aspirator nozzles on the sink faucets. When a stoppered vacuum flask is attached to one of these vacuum sources the number of collisions of gas inside the flask decreases thus decreasing the pressure. Temperature in science is measured using the Celsius ( o C) and Kelvin (K) scales. Celsius and Kelvin degrees measure the same quantity, (a Celsius degree and a Kelvin degree are the same size) they just start at different points, (K = o C + 273). When solving mathematical problems involving temperature, the units must always be in Kelvin. The common temperatures of the daily weather reports in the United States are reported using the Fahrenheit ( o F) scale which is not used in science. The volumes of solids and liquids are only minimally affected by pressure (P) or Temperature (T). Gases, however, behave much differently than solids or liquids in that their Volume (V) significantly expands or contracts with changes in Pressure (P) and Temperature (T).

2 2 SOLUBILITY: Gases, like some solids or liquids, are able to dissolve partially in water. Some gases, such as Oxygen (O2), Nitrogen (N2), or Carbon Dioxide (CO2) easily dissolve in water. We say these are soluble gases. However, some gases such as Helium (He) dissolve only a little bit. Gases that do not dissolve in water very much are said to be either insoluble or partially soluble depending on just how much does dissolve. Unlike the solubility of solids or liquids, the ability of gases to dissolve in water (the solubility of gases) changes if either the surrounding pressure or the surrounding temperature changes. In the laboratory exercises that follow you will discover the relationships between Pressure (P), Temperature (T) and the Solubility of a gas, and be able to derive Henry s Law for yourself. DIRECT VS. INVERSE RELATIONSHIPS: When one property (property A) influences another property (property B) to change there are two possibilities for how the change could occur. A direct relationship between properties means that if property A increases (goes up) then property B increases (goes up) also; Or likewise, if A decreases (goes down) then B also decreases (goes down). Properties A and B in a direct relationship are like 2 sides of a barbell. When a weight-lifter raises or lowers the bar both A and B move up or down together. An inverse or indirect relationship between properties means that if property A increases (goes up) then property B decreases (goes down); Or likewise, if A decreases (goes down) then B increases (goes up). Properties A and B in an inverse relationship are like 2 sides of a seesaw. When one side goes down, the other goes up. Of course not every property is related to every other property. Sometimes events are totally unrelated. The scientific method and analysis of experimental testing can help to determine if properties are related or not. In the laboratory exercises that follow you will discover the relationships between Volume (V), Pressure (P), and Temperature (T) and be able to derive Boyle s Law and Charles Law of gases for yourself.

3 3 PROCEDURES: ACTIONS: VACUUM: 1. Attach a 250 ml vacuum flask to the benchtop vacuum line or to the side arm of your sink aspirator using heavy walled tubing. 2. Place the palm of your hand over the top of the vacuum flask and then turn on the vacuum line or aspirator water full force. Observe the effect of the vacuum on your hand. Vacuum flask Complete the report sheet indicating on the inside and outside of the flask the locations of high pressure (P ) with up arrows, and locations of low pressure (P ) with down arrows. I. BOYLE S LAW: VOLUME VS PRESSURE 1. Slightly inflate a small balloon just large enough so that it can be placed inside your 250 ml vacuum flask. Knot it tightly, and insert the balloon into the vacuum flask. Cap the flask tightly with a rubber stopper. 2. Turn on your vacuum source full force. On the report sheet (IA) record your observations. 3. If using a vacuum line turn off the vacuum and detach the vacuum tubing from the vacuum source to let atmospheric pressure into the vacuum flask. Record your observations (IB). 4. Repeat steps 2-4, only instead of a balloon use a marshmallow inside the flask. Report your results (IAA & IBB). PHYSIOLOGICAL APPLICATION: BREATHING 5. Hold a bell jar lung demonstration model and gently pull out on the thin rubber diaphragm. Observe and record (IIC) the behavior of the lung balloons. 6. Now, gently press in on the rubber diaphragm. Observe and record (IID) the behavior of the lung balloons. 7. Sit or stand up straight and put your hand on your diaphragm muscle just below your rib cage. 8. With your hand on your diaphragm and without raising your shoulders breathe in deeply. Observe and record the behavior of your diaphragm muscle as you expand your lung volume. (IE)

4 4 Formulate Boyle s law by summarizing your results in the blanks given on the report sheet. (IF) II. CHARLES LAW: VOLUME VS TEMPERATURE 1. Take a glass capillary tube that has been sealed at one end. Using a tiny dropper or syringe with a blunt needle, inject a drop of colored water into the center of the tube so that air is trapped inside the tube. 2. Holding the tube of trapped air near the mouth of the tube, carefully draw a line at the lower edge of the colored water with a marking pencil. 3. Hold the tube at the top, above the marked line, and immerse it in a beaker of ice water. Observe the pocket of trapped air and record your results on the report sheet. (IIA) 4. Now, take the tube out of the ice water and immerse it in a beaker of hot tap water. Observe the pocket of trapped air and record your results on the report sheet. (IIB) 5. Dispose of the glass capillary tube in the glass or sharps waste container. PRACTICAL APPLICATION: IMPLODING CAN B1. Place an aluminum pop can containing about 1 inch of water on a hot plate or over a flame. B2. Heat until steam (gaseous water) steadily comes from the can. B3. With large tongs or a folded paper towel strip, remove the steaming can from the heat source and immediately invert into a bucket of ice water. Observe the effects. B4. Record your observations of both heating (IIIC) and cooling (IIID) on the report sheet. 6. Formulate Charles Law by summarizing your results in the space provided on the report sheet. (IIE) III. HENRY S LAW: SOLUBILITY VS PRESSURE 1. Pour ice cold carbonated water (CO2 dissolved in H2O) into a vacuum flask to a level of about 1 inch. 2. Set the tightly stoppered flask in an ice water bath to keep it cold. 3. Connect the flask to the vacuum source and turn it on full force. On the report sheet (IIIA) record your observations. Indicate increasing solubility

5 5 (Ability of gas to dissolve) (S ) of CO2 gas with up arrows, and decreasing solubility (S ) of CO2 gas with down arrows. 4. Turn off the vacuum source and detach the vacuum tubing to allow the flask to return to atmospheric pressure. Record your observations. (IIIB) 5. Formulate Henry s Law by summarizing your results in the space provided on the report sheet. (IIIE) PHYSIOLOGICAL APPLICATION: THE BENDS 6. Now that you have discovered Henry s law, imagine what would happen to the solubility (S) of air (oxygen and nitrogen gases) in the blood (a water solution) of a diver that descends to the depths of the ocean (P ). Record your hypothetical results (IIIC). Now imagine that the diver in the depths of the ocean quickly rises to the surface. What happens to the atmospheric pressure and what happens to the solubility of gases in the blood? Record your hypothetical results (IIID)

6 6

7 7 PROPERTIES OF GASES: REPORT: NAME DATE I. BOYLE S LAW: VOLUME VS PRESSURE Action Observations Effect on Pressure P or P A. Vacuum source turned on with balloon in flask. Effect on Volume V or V B. Vacuum hose detached with balloon in flask. AA. Vacuum source turned on with marshmallow in flask. BB. Vacuum hose detached with marshmallow in flask. C. Model diaphragm muscle contracted (pulled down) Bell Jar P Lung V D. Model diaphragm muscle relaxed (pushed in) Bell Jar P Lung V E. Inhale deeply Diaphragm muscle was Contracted or Relaxed (circle one) Chest cavity P Lung V F. Conclusion: 1. The volume of a gas as the pressure. A. decreases, increases B. increases, increases. C. does not change, changes 2. Boyle s Law: The volume of a gas the pressure. A. varies directly with B. varies inversely with C. is unrelated to

8 8 II. CHARLES LAW: VOLUME VS TEMPERATURE Action Observations Effect on Temperature T or T A. Trapped air immersed in ice water. Effect on Volume V or V B. Trapped air immersed in hot water. C. Hot water vapor heated pop can D. Hot water vapor cooling pop can E. Conclusion: 1. The volume of a gas as the temperature. A. decreases, increases B. increases, increases. C. does not change, changes 2. Charles Law: The volume of a gas the temperature. A. varies directly with B. varies inversely with C. is unrelated to

9 9 III. HENRY S LAW: SOLUBILITY VS PRESSURE Action Observations Effect on Pressure A. Vacuum source turned on with carbonated solution in flask. B. Vacuum hose detached with carbonated solution in flask. C. A diver is deep in the ocean with gases dissolved in the blood D. A diver, deep in the ocean with gases dissolved in the blood, comes rapidly to the surface. P or P Effect on gas Solubility S or S E. Conclusion: 1. The solubility of a gas in water (the ability of a gas to dissolve) as the pressure. A. decreases, increases B. increases, increases. C. does not change, changes 2. Henry s Law: The solubility of a gas the pressure. A. varies directly with B. varies inversely with C. is unrelated to

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