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THE SOLUBILITY of GASES in LIQUIDS Introductory Information C
THE SOLUBILITY OF GASES IN LIQUIDS Introductory Information C. L. Young, R. Battino, and H. L. Clever INTRODUCTION The Solubility Data Project aims to make a comprehensive search of the literature for data on the solubility of gases, liquids and solids in liquids. Data of suitable accuracy are compiled into data sheets set out in a uniform format. The data for each system are evaluated and where data of sufficient accuracy are available values are recommended and in some cases a smoothing equation is given to represent the variation of solubility with pressure and/or temperature. A text giving an evaluation and recommended values and the compiled data sheets are published on consecutive pages. The following paper by E. Wilhelm gives a rigorous thermodynamic treatment on the solubility of gases in liquids. DEFINITION OF GAS SOLUBILITY The distinction between vapor-liquid equilibria and the solubility of gases in liquids is arbitrary. It is generally accepted that the equilibrium set up at 300K between a typical gas such as argon and a liquid such as water is gas-liquid solubility whereas the equilibrium set up between hexane and cyclohexane at 350K is an example of vapor-liquid equilibrium. However, the distinction between gas-liquid solubility and vapor-liquid equilibrium is often not so clear. The equilibria set up between methane and propane above the critical temperature of methane and below the criti cal temperature of propane may be classed as vapor-liquid equilibrium or as gas-liquid solubility depending on the particular range of pressure considered and the particular worker concerned. -
Dysbarism - Barotrauma
DYSBARISM - BAROTRAUMA Introduction Dysbarism is the term given to medical complications of exposure to gases at higher than normal atmospheric pressure. It includes barotrauma, decompression illness and nitrogen narcosis. Barotrauma occurs as a consequence of excessive expansion or contraction of gas within enclosed body cavities. Barotrauma principally affects the: 1. Lungs (most importantly): Lung barotrauma may result in: ● Gas embolism ● Pneumomediastinum ● Pneumothorax. 2. Eyes 3. Middle / Inner ear 4. Sinuses 5. Teeth / mandible 6. GIT (rarely) Any illness that develops during or post div.ing must be considered to be diving- related until proven otherwise. Any patient with neurological symptoms in particular needs urgent referral to a specialist in hyperbaric medicine. See also separate document on Dysbarism - Decompression Illness (in Environmental folder). Terminology The term dysbarism encompasses: ● Decompression illness And ● Barotrauma And ● Nitrogen narcosis Decompression illness (DCI) includes: 1. Decompression sickness (DCS) (or in lay terms, the “bends”): ● Type I DCS: ♥ Involves the joints or skin only ● Type II DCS: ♥ Involves all other pain, neurological injury, vestibular and pulmonary symptoms. 2. Arterial gas embolism (AGE): ● Due to pulmonary barotrauma releasing air into the circulation. Epidemiology Diving is generally a safe undertaking. Serious decompression incidents occur approximately only in 1 in 10,000 dives. However, because of high participation rates, there are about 200 - 300 cases of significant decompression illness requiring treatment in Australia each year. It is estimated that 10 times this number of divers experience less severe illness after diving. Physics Boyle’s Law: The air pressure at sea level is 1 atmosphere absolute (ATA). Alternative units used for 1 ATA include: ● 101.3 kPa (SI units) ● 1.013 Bar ● 10 meters of sea water (MSW) ● 760 mm of mercury (mm Hg) ● 14.7 pounds per square inch (PSI) For every 10 meters a diver descends in seawater, the pressure increases by 1 ATA. -
Nitrogen Narcosis
WHAT IS IT? A reversible alteration in consciousness that occurs while at depth (usually noticeable around 30 meters or 100 ft) Caused by the anesthetic effect of certain gases at high pressure NITROGEN NARCOSIS Depths Beyond 100 Feet! Individual Variability Day-to-Day Variability Signs and Symptoms of N2 Narcosis Impaired performance mental/manual work Dizziness, euphoria, intoxication Overconfidence Uncontrolled laughter Overly talkative Memory loss/post-dive amnesia Perceptual narrowing Impaired sensory function Loss of consciousness > 300 ft Deep Scuba Dives Breathing Air YEAR DIVER DEPTH 1943 Dumas 203 feet 1948 Dumas 307 feet 1967 Watts 390 feet 1968 Watson 437 feet 1989 Gilliam 452 feet Prevention of Nitrogen Narcosis Restrict diving depth to less than 100 fsw If affected, return immediately to surface Plan dive beforehand − Max time to be on bottom − Any decompression required − Minimum air required for ascent − Emergency action in event of accident Breathe helium/oxygen mixture How to Beat Narcosis (Francis 2006) Be sober, no hangover and drug free Be rested and confident Use a high quality regulator Avoid task loading Be over trained Approach limits gradually Use a slate to plan dive Schedule gauge checks and buddy checks Be positive, well motivated and prudent Oxygen Characteristics: − Colorless − Odorless − Tasteless Disadvantage: − Toxic when Oxygen is the only gas excessive amounts metabolized by the human body are breathed under pressure Too much or too little oxygen is dangerous! Oxygen Toxicity -
AP Chemistry Chapter 5 Gases Ch
AP Chemistry Chapter 5 Gases Ch. 5 Gases Agenda 23 September 2017 Per 3 & 5 ○ 5.1 Pressure ○ 5.2 The Gas Laws ○ 5.3 The Ideal Gas Law ○ 5.4 Gas Stoichiometry ○ 5.5 Dalton’s Law of Partial Pressures ○ 5.6 The Kinetic Molecular Theory of Gases ○ 5.7 Effusion and Diffusion ○ 5.8 Real Gases ○ 5.9 Characteristics of Several Real Gases ○ 5.10 Chemistry in the Atmosphere 5.1 Units of Pressure 760 mm Hg = 760 Torr = 1 atm Pressure = Force = Newton = pascal (Pa) Area m2 5.2 Gas Laws of Boyle, Charles and Avogadro PV = k Slope = k V = k P y = k(1/P) + 0 5.2 Gas Laws of Boyle - use the actual data from Boyle’s Experiment Table 5.1 And Desmos to plot Volume vs. Pressure And then Pressure vs 1/V. And PV vs. V And PV vs. P Boyle’s Law 3 centuries later? Boyle’s law only holds precisely at very low pressures.Measurements at higher pressures reveal PV is not constant, but varies as pressure varies. Deviations slight at pressures close to 1 atm we assume gases obey Boyle’s law in our calcs. A gas that strictly obeys Boyle’s Law is called an Ideal gas. Extrapolate (extend the line beyond the experimental points) back to zero pressure to find “ideal” value for k, 22.41 L atm Look Extrapolatefamiliar? (extend the line beyond the experimental points) back to zero pressure to find “ideal” value for k, 22.41 L atm The volume of a gas at constant pressure increases linearly with the Charles’ Law temperature of the gas. -
THE SOLUBILITY of GASES in LIQUIDS INTRODUCTION the Solubility Data Project Aims to Make a Comprehensive Search of the Lit- Erat
THE SOLUBILITY OF GASES IN LIQUIDS R. Battino, H. L. Clever and C. L. Young INTRODUCTION The Solubility Data Project aims to make a comprehensive search of the lit erature for data on the solubility of gases, liquids and solids in liquids. Data of suitable accuracy are compiled into data sheets set out in a uni form format. The data for each system are evaluated and where data of suf ficient accuracy are available values recommended and in some cases a smoothing equation suggested to represent the variation of solubility with pressure and/or temperature. A text giving an evaluation and recommended values and the compiled data sheets are pUblished on consecutive pages. DEFINITION OF GAS SOLUBILITY The distinction between vapor-liquid equilibria and the solUbility of gases in liquids is arbitrary. It is generally accepted that the equilibrium set up at 300K between a typical gas such as argon and a liquid such as water is gas liquid solubility whereas the equilibrium set up between hexane and cyclohexane at 350K is an example of vapor-liquid equilibrium. However, the distinction between gas-liquid solUbility and vapor-liquid equilibrium is often not so clear. The equilibria set up between methane and propane above the critical temperature of methane and below the critical temperature of propane may be classed as vapor-liquid equilibrium or as gas-liquid solu bility depending on the particular range of pressure considered and the par ticular worker concerned. The difficulty partly stems from our inability to rigorously distinguish between a gas, a vapor, and a liquid, which has been discussed in numerous textbooks. -
CEE 370 Environmental Engineering Principles Henry's
CEE 370 Lecture #7 9/18/2019 Updated: 18 September 2019 Print version CEE 370 Environmental Engineering Principles Lecture #7 Environmental Chemistry V: Thermodynamics, Henry’s Law, Acids-bases II Reading: Mihelcic & Zimmerman, Chapter 3 Davis & Masten, Chapter 2 Mihelcic, Chapt 3 David Reckhow CEE 370 L#7 1 Henry’s Law Henry's Law states that the amount of a gas that dissolves into a liquid is proportional to the partial pressure that gas exerts on the surface of the liquid. In equation form, that is: C AH = K p A where, CA = concentration of A, [mol/L] or [mg/L] KH = equilibrium constant (often called Henry's Law constant), [mol/L-atm] or [mg/L-atm] pA = partial pressure of A, [atm] David Reckhow CEE 370 L#7 2 Lecture #7 Dave Reckhow 1 CEE 370 Lecture #7 9/18/2019 Henry’s Law Constants Reaction Name Kh, mol/L-atm pKh = -log Kh -2 CO2(g) _ CO2(aq) Carbon 3.41 x 10 1.47 dioxide NH3(g) _ NH3(aq) Ammonia 57.6 -1.76 -1 H2S(g) _ H2S(aq) Hydrogen 1.02 x 10 0.99 sulfide -3 CH4(g) _ CH4(aq) Methane 1.50 x 10 2.82 -3 O2(g) _ O2(aq) Oxygen 1.26 x 10 2.90 David Reckhow CEE 370 L#7 3 Example: Solubility of O2 in Water Background Although the atmosphere we breathe is comprised of approximately 20.9 percent oxygen, oxygen is only slightly soluble in water. In addition, the solubility decreases as the temperature increases. -
Ideal Gasses Is Known As the Ideal Gas Law
ESCI 341 – Atmospheric Thermodynamics Lesson 4 –Ideal Gases References: An Introduction to Atmospheric Thermodynamics, Tsonis Introduction to Theoretical Meteorology, Hess Physical Chemistry (4th edition), Levine Thermodynamics and an Introduction to Thermostatistics, Callen IDEAL GASES An ideal gas is a gas with the following properties: There are no intermolecular forces, except during collisions. All collisions are elastic. The individual gas molecules have no volume (they behave like point masses). The equation of state for ideal gasses is known as the ideal gas law. The ideal gas law was discovered empirically, but can also be derived theoretically. The form we are most familiar with, pV nRT . Ideal Gas Law (1) R has a value of 8.3145 J-mol1-K1, and n is the number of moles (not molecules). A true ideal gas would be monatomic, meaning each molecule is comprised of a single atom. Real gasses in the atmosphere, such as O2 and N2, are diatomic, and some gasses such as CO2 and O3 are triatomic. Real atmospheric gasses have rotational and vibrational kinetic energy, in addition to translational kinetic energy. Even though the gasses that make up the atmosphere aren’t monatomic, they still closely obey the ideal gas law at the pressures and temperatures encountered in the atmosphere, so we can still use the ideal gas law. FORM OF IDEAL GAS LAW MOST USED BY METEOROLOGISTS In meteorology we use a modified form of the ideal gas law. We first divide (1) by volume to get n p RT . V we then multiply the RHS top and bottom by the molecular weight of the gas, M, to get Mn R p T . -
Outta Gas (From the 2007: Exploring the Inner Space of the Celebes Sea
2007: Exploring the Inner Space of the Celebes Sea Outta Gas FOCUS MAXIMUM NUMBER OF STUDENTS Gas laws 30 GRADE LEVEL KEY WORDS 9-12 (Chemistry/Physics) Celebes Sea SCUBA diving FOCUS QUESTION Gas laws How can Boyle’s Law, Charles’ Law, Gay-Lussac’s Ideal Gas Law Law, Henry’s Law, and Dalton’s Law be used to Boyle’s Law predict the behavior of gases used in SCUBA div- Charles’ Law ing? Gay-Lussac’s Law Henry’s Law LEARNING OBJECTIVES Dalton’s Law Students will define Boyle’s Law, Charles’ Law, Pressure Gay-Lussac’s Law, Henry’s Law, and Dalton’s Law. Worksheet Mathematics Students will use Boyle’s Law, Charles’ Law, Gay- Lussac’s Law, Henry’s Law, and Dalton’s Law to BACKGROUND INFORMATION solve practical problems related to SCUBA diving. Indonesia is well-known as one of Earth’s major centers of biodiversity. Although Indonesia cov- MATERIALS ers only 1.3 percent of Earth’s land surface, it “Blue Water Diving Worksheet,” one copy for includes: each student or student group • 10 percent of the world’s flowering plant species; AUDIO/VISUAL MATERIALS • 12 percent of the world’s mammal species; None • 16 percent of all reptile and amphibian species; and TEACHING TIME • 17 percent of the world’s bird species. One or two 45-minute class periods plus time for students to complete worksheet In addition, together with the Philippines and Great Barrier Reef, this region has more species SEATING ARRANGEMENT of fishes, corals, mollusks, and crustaceans than Classroom style any other location on Earth. -
Chapter 14: Gases
418-451_Ch14-866418 5/9/06 6:19 PM Page 418 CHAPTER 14 Gases Chemistry 2.a, 3.c, 3.d, 3.e, 4.a, 4.c, 4.d, 4.e, 4.f, 4.g, 4.h I&E 1.b, 1.c, 1.d What You’ll Learn ▲ You will use gas laws to cal- culate how pressure, tem- perature, volume, and number of moles of a gas will change when one or more of these variables is altered. ▲ You will compare properties of real and ideal gases. ▲ You will apply the gas laws and Avogadro’s principle to chemical equations. Why It’s Important From barbecuing on a gas grill to taking a ride in a hot-air balloon, many activities involve gases. It is important to be able to predict what effect changes in pressure, temperature, volume, or amount, will have on the properties and behavior of a gas. Visit the Glencoe Chemistry Web site at chemistrymc.com to find links about gases. Firefighters breathe air that has been compressed into tanks that they can wear on their backs. 418 Chapter 14 418-451_Ch14-866418 5/9/06 6:19 PM Page 419 DISCOVERY LAB More Than Just Hot Air Chemistry 4.a, 4.c I&E 1.d ow does a temperature change affect the air in Ha balloon? Safety Precautions Always wear goggles to protect eyes from broken balloons. Procedure 1. Inflate a round balloon and tie it closed. 2. Fill the bucket about half full of cold water and add ice. 3. Use a string to measure the circumference of the balloon. -
Gases Boyles Law Amontons Law Charles Law ∴ Combined Gas
Gas Physics FICK’S LAW Adolf Fick, 1858 Properties of “Ideal” Gases Fick’s law of diffusion of a gas across a fluid membrane: • Gases are composed of molecules whose size is negligible compared to the average distance between them. Rate of diffusion = KA(P2–P1)/D – Gas has a low density because its molecules are spread apart over a large volume. • Molecules move in random lines in all directions and at various speeds. Wherein: – The forces of attraction or repulsion between two molecules in a gas are very weak or negligible, except when they collide. K = a temperature-dependent diffusion constant. – When molecules collide with one another, no kinetic energy is lost. A = the surface area available for diffusion. • The average kinetic energy of a molecule is proportional to the absolute temperature. (P2–P1) = The difference in concentraon (paral • Gases are easily expandable and compressible (unlike solids and liquids). pressure) of the gas across the membrane. • A gas will completely fill whatever container it is in. D = the distance over which diffusion must take place. – i.e., container volume = gas volume • Gases have a measurement of pressure (force exerted per unit area of surface). – Units: 1 atmosphere [atm] (≈ 1 bar) = 760 mmHg (= 760 torr) = 14.7 psi = 0.1 MPa Boyles Law Amontons Law • Gas pressure (P) is inversely proportional to gas volume (V) • Gas pressure (P) is directly proportional to absolute gas • P ∝ 1/V temperature (T in °K) ∴ ↑V→↓P ↑P→↓V ↓V →↑P ↓P →↑V • 0°C = 273°K • P ∝ T • ∴ P V =P V (if no gas is added/lost and temperature -
The Behavior and Applications of Gases
329670_ch10.qxd 07/20/2006 11:32 AM Page 394 The Behavior and Applications Contents and Selected Applications 10.1 The Nature of Gases of Gases 10.2 Production of Hydrogen and the Meaning of Pressure 10.3 Mixtures of Gases—Dalton’s Law and Food Packaging Chemical Encounters: Dalton’s Law and Food Packaging 10.4 The Gas Laws—Relating the Behavior of Gases to Key Properties Chemical Encounters: Balloons and Ozone Analysis 10.5 The Ideal Gas Equation 10.6 Applications of the Ideal Gas Equation Earth’s atmosphere is a very thin layer of gases (only 560 km thick) that surrounds Chemical Encounters: Automobile Air Bags Chemical Encounters: Acetylene the planet. Although the atmosphere makes up only a small part of our planet, 10.7 Kinetic-Molecular Theory it is vital to our survival. 10.8 Effusion and Diffusion 10.9 Industrialization: A Wonderful, Yet Cautionary, Tale Chemical Encounters: Ozone Chemical Encounters: The Greenhouse Effect 394 329670_ch10.qxd 6/19/06 1:45 PM Page 395 Our planet is surrounded by a relatively thin layer known as an atmosphere. It supplies all living organisms on Earth with breathable air, serves as the vehicle to deliver rain to our crops, and protects us from harmful ultraviolet rays from the Sun. Although it does contain solid particles, such as dust and smoke, and liquid droplets, such as sea TABLE 10.1 Composition of Dry Air spray and clouds, much of the atmosphere we live in is Percent Parts per Million actually a mixture of the gases shown in Table 10.1. -
Nitrogen Narcosis in Hyperbaric Chamber Nurses
International Journal of Research in Nursing Original Research Paper Nitrogen Narcosis in Hyperbaric Chamber Nurses 1,2 Denise F. Blake, 3Derelle A. Young and 4Lawrence H. Brown 1Emergency Department, The Townsville Hospital, Douglas, Queensland, Australia 2School of Marine and Tropical Biology, James Cook University, Townsville, Queensland, 4814, Australia 3Hyperbaric Medicine Unit, The Townsville Hospital, Townsville, Queensland, Australia 4Mount Isa Centre for Rural and Remote Health, Faculty of Medicine, Health and Molecular Sciences, James Cook University, Townsville, QLD, 4814, Australia Article history Abstract: Hyperbaric nursing has become a specialty requiring high skill Received: 24-09-2014 and knowledge. Nitrogen narcosis is a perceived risk for all inside Revised: 03-10-2014 hyperbaric chamber nurses. The actual degree of impairment at pressure Accepted: 16-12-2015 has not been quantified. Twenty eight subjects participated in the study. Sixteen hyperbaric nurse candidates and five experienced hyperbaric Corresponding Author: Denise F. Blake, nurses completed Trail Making Test A (TMTA) pre and post compression Emergency Department, and at 180 kPa and 300 kPa. Seven experienced hyperbaric staff acted as The Townsville Hospital, an unpressurized reference. Time to completion of the test was recorded in Douglas, Queensland, Australia seconds; pre-test anxiety and perceived symptoms of narcosis at 300 kPa Email: [email protected] were also recorded. There were no statistically significant differences in the corrected TMT A times at the four different time periods. There was a trend to poorer performance by the nurse candidates at 180 kPa however this was not statistically significant. Most subjects felt some degree of narcosis at 300 kPa.