How Gas Laws Apply In the Health Care Industry - Research Paper Example

? How Gas Laws Apply In the Health Care Industry No: How Gas Laws Apply In the Health Care Industry Introduction Gas laws play a significant role in everyday life. The laws have a significant influence on the lives of living organisms. The atmospheric pressure, respiratory system of living organisms, etc all work according to the ideas detailed in the gas laws. Under an uncontrollable condition, gas a high-pressurized gas can be as dangerous as a nothing in the world. Most of the arms and ammunition works utilizing the principles of the gas laws. A bullet utilized the gas pressure to be shot from the bullet. This high pressure is attained by igniting the gunpowder present in the bullet. Rockets also have the same principle but a rocket requires a lot more fuel to attain such a pressure due to its weight as compared to a bullet. In this way, the significance of the gas laws is in every aspect of life. Gas laws are applicable to most of the industries to provide goods and services to the customers. Gas Gas is a state of matter in which the molecules of the matter remains apart from each other, in this way, the volume of the gas remains higher as compared to its weight. Gas may be colorless and odorless but gases have odor and slightly light color like chlorine has a stingy smell while oxygen is colorless and odorless (West 2008). Difference between Gas and Other Type of Matter The other two states of matter are solid and liquid. The molecules of the solids are such liked to each other that the molecules can only vibrate maintaining their position because of external force. In liquids, the molecules are liked to each other but in relatively loose bond than that of the solids. In this way, the molecules can more from one place to remains contacted with the other molecules. In gases, the moles are free to move, there exists no bondage between the molecules of the gas. Gas molecules of a gas (element) move freely in open atmosphere making a mixture with the gas molecules of other gases (Jennet 2004). Volume Volume is an amount of gas that represents the amount of gas in a container. Volume is measured in the litters, mm3, dm3 and cm3.other than gaseous compounds, volume is the product of three dimensions namely length, width and height. Pressure Pressure is a term, which is utilized when the freely moving particles of the gas collide with the walls of the container and collide with each other to make a force exerting against the wall of the container. The more the dimensions of the container, the lesser will be the pressure and the container with less dimensions has the more pressure for the same amount of gas. In the similar way, if the amount of gas is increases the pressure will be increased in the container with similar dimensions. The units of the pressure are Atmospheres (atm), Pounds per square inch (PSI), Inches of mercury (in.Hg) and millimeters of mercury (mm.Hg). While the SI unit of pressure is Pascal (Pa) or Newton per square meter (N/m2) while non SI units are Bar and dyne per square centimeter (barye). Standard pressure is considered as one atm (Halzner 2011). Temperature Temperature intensely affects a gas. Temperature is an external effect that affects the molecular motion of the gas particles. As the temperature increases the random molecular motion of the particles, increases as the gas molecules take the heat energy and convert it to kinetic energy. In this way, the volume of the gas increases and thus the pressure increases. Similarly, if a container filled with an amount of gas is exposed to extreme lower temperature, the gas in the container contracts and creates a vacuum in the container, the container may sucker external gas to fill the vacuum. The standard value of temperature is 273K or 0oC. The units of temperature are Kelvin (K), Celsius (C) (Halliday, Resnick and Walker 2005). Chemical amount The chemical amount of gas is represented as the no of grams or no of moles. The amount in grams is calculated using the chemical formula of the gas. The amount in moles is calculated by dividing the given amount by the molecular mass in grams. Moles (mol) represent the amount in moles and g represents the amount in grams. Avogadro’s number Avogadro’s number is the key content attained from the Avogadro’s Law, which has a view that at standard temperature, and pressure (STP) the number of molecules of every gas remains the same if the volume remains constant. The law states “Volume of a gas is directly proportional to the number moles of the gas” and two gases having similar volumes have equal number of molecules similarly two gases having similar number of molecular have same volumes (Shipman, Wilson and Todd 2009). By Avogadro’s Law: V ? n, where V is volume of gas and n is the number of moles of a gas. The number of atoms ions or molecules that a gas is 6.022x1023 molecules/mol, where Temperature remains at 273K or 0oC, pressure remains at 1 atm, and volume remains at 22.4dm3. Association between Volume, Temperature and Pressure Volume, Temperature and Pressure are highly associated with each other and depend on each other. As the pressure of a gas increases the volume of gas decreases and as the temperature increases pressure increases. The increase or decrease in one quantity influence the other quantity to increases or decrease. The association can be easily defined in the gas laws. Gas Laws Gas laws are the laws that govern with different properties of the gas. Gas law also represent an association among the different variables of the gas like pressure, temperature and pressure. Gas laws indicates how the different variables of the gas are associated with each other. Boyles Law The Scientists ‘Robert Boyle’ discovered Boyles Law in 1662. The law states “Pressure is inversely proportional to the volume” (Holbrow, Lloyd, Amato, Galvez and Parks 2010), if the temperature remains constant in a closed container. Both the volume and the pressure are inverse quantities. If any one of the quantity increases, the other one decreases. If pressure is P and volume is V then by the Boyle’s law: P ? 1/V or V ? 1/P (Temperature remains constant) Alternatively, PV=k, where k is a constant in the system. The law can also be utilized to find out the initial and final conditions on pressures and volumes. The law can determine the change in one quantity as the result of increasing or decreasing the other quantity. In this way: P1V1=P2V2, where P1 and V1 represents the initial pressure and volume while P2 and V2 represents the finial pressure and volume. Charles Law Jacques Charles presented Charles’s law around 1780’s. The law shows the association between the temperature and volume. Charles’s law states “Volume is directly proportional to the temperature” if pressure of the gas remains constant (Zumdahl 2004). Both the quantities are directly linked to each other and if one quantity increases the other one, increases too. The temperature increase the mean kinetic energy of the gas particles and thus the particles collide with the walls of the container and with each other rapidly and exerts more force thus results in increases in the volume. If V is the Volume of gas and T is the temperature that is given to the gas, the Charles’s law can be written as: V ? T (where pressure remains constant) Alternatively, V/T=k, where k is a constant of proportionality. Charles’s law can also be utilized to find out the initial and final conditions of temperature and volumes. The law can determine the change in one quantity as the result of increasing or decreasing the other quantity. In this way: V1 /T1=V2 /T2, where T1 and V1 represents the initial Temperature and volume while T2 and V2 represents the finial temperatures and volume. Combined Gas Law The combination of the two laws, Charles’s law and Boyle’s law gives the combined gas law that utilized both the characteristics of the Charles law and the Boyle’s law. The combined gas law states that the product of pressure and volume of a gas divided by the temperature remains constant. If P and V are the Pressure and Volume of the gas respectively and T is the temperature of gas, the combined gas law can be written as: PV/T= k (where k is a constant) Combined gas law can also be utilized to find out the initial and final conditions of pressure, temperature and volumes. The law can determine the change in one quantity as the result of increasing or decreasing the other quantities. In this way: P1V1 /T1= P2V2 /T2, where P1, T1 and V1 represents the initial pressure, temperature and volume while P2, T2 and V2 represents the finial pressure, temperatures and volume. Gay-Lussac’s Law Chemist Joseph Louis Gay-Lussac presented the Gay-Lussac’s law, which showed the association between the pressure and the temperature. The law showed that the pressure of a gas has a direct relation with the temperature, if volume of the contained remains constant. If temperature to the container increases, the pressure of the gas inside the container increases (Holbrow, Lloyd, Amato, Galvez and Parks 2010). The law can also be transformed as the ratio of the pressure and temperature remains constant. If P is the pressure of the gas and T is the temperature that is given to the gas then according to the Gay-Lussac’s law: P ? T (Volume of the container remains constant) Alternatively, P/T= k (where k is the constant) Gay-Lussac’s gas law can also be utilized to find out the initial and final conditions of pressure and temperature. The law can determine the change in one quantity as the result of increasing or decreasing the other quantity. In this way: P1 /T1= P2 /T2, where P1 and T1 represents the initial pressure and temperature while P2 andT2 represents the finial pressure and temperatures. Ideal Gas Law Ideal gas law is the resultant from the combination the two gas laws that are Boyle’s law and Charles law. According to the ideal gas law, the product of the pressure and volume of a gas is directly related to the product of number of moles of the gas and temperature given to the gas. It is also referred as the gas obeying the all the laws like Charles’s law, Boyle’s law, Avogadro’s law and Gay-Lussac Law (Kotz, Treichel, Townsend and Raymond 2009). If V is the volume of the gas, P is the pressure of the gas, n is the number of moles of gas and T is the temperature given to the gas, As by Boyle’s law: V ? 1/P (Temperature remains constant) By Charles’s law: V ? P (Temperature remains constant) By Gay-Lussac’s law: P ? T (Volume remains constant) Then the ideals gas law can be written as: PV ? n T or V ? n T/P Alternatively, PV=n RT, where R is universal gas constant. It can also be written as: PV =N kT, where N is the number of molecules of the gas and k is the Boltzmann’s constant. Gas Laws and Human Bodies Gas laws are highly related to the human bodies, as the vital functions of the body are incomplete without applying the gas laws. The main function of the body that is most influenced by the characteristics of gas law is the human’s respiratory system. Each cell of our body respire utilizing the air around us and then extracting oxygen from the atmosphere and maintaining a certain breathing pressure in the lungs. a) Normal Functions i) Breathing Breathing involves the contraction and relaxation of lungs and diaphragm. The diaphragm moves down in order to make a space for the air to suck into the lungs and fill the low pressure in the lungs. After that, the diaphragm mover up and compresses the lungs thus increase the pressure in the lungs as compared to its volume and lungs expels the air out thus implementing the Boyle’s law. There exists a little difference of pressures or air taken in and out. The pressure exceeds not more than three torr (Kotz, Treichel, Townsend and Raymond 2009). Similarly, temperature has also high impact on the volume of air. If the temperature of the air we take in more, the more volume of air is required to provide us the required oxygen. ii) Blood Pressure The respiratory system is highly linked with the blood circulation system. It is the blood, which circulates the oxygen to each cell of our body by maintaining a certain blood pressure. If the blood pressure remains low, then most of cells of the body may not get the required oxygen. If the blood remains high, the small capillaries will burst. In this way, body needs to maintain a constant blood pressure. A blood is a liquid and oxygen in the blood is in the form of oxy-hemoglobin, the breathing system is associated with the blood pressure and thus the gas laws. iii) Heart Beat Heartbeat is a function of heart to pump the blood to the body. Blood not only provides oxygen to the organs and cells but also provides them with nutrition. Heart is made up of muscles tissues, which are dedicated to maintain a blood pressure by contracting and relaxing. When the muscles contracts the blood flows out of the heart and when the it relaxes, it allows its space to be filled by the blood, while lungs sucks the carbon dioxide from the blood and give blood oxygen. b) Abnormal Occurrences i) Decompression Sickness Decompression sickness is a type of illness that is caused due to interaction with the higher pressures as the deep-sea divers face this problem as the pressure inside the water increases as the depth of water increases. If at sea level, the pressure is one atmosphere then at 40 feet, the divers may have the pressure of four times the pressure at sea level (Dombrink and Tanis 1983). At this pressure, the nitrogen bubbles and other compounds penetrate into the blood and if the diver does not know what to do in such a condition, the illness may cause bone, joint and muscles pain. The gas also follows the Henry’s law that states, “The amount of gas that will dissolve in a liquid at a given temperature varies directly with the pressure above the liquid” (Dombrink and Tanis 1983). In order to cure the Decompression sickness, the divers must have to stay in a recompression chamber that slowly decreases the pressure down to the atmospheric pressure. ii) Others At higher altitudes, where the pressure lowers to a little value, the ears drums may stop working. All the organs that have an association with the flow of air may stop working as they work on the sea level. In unpressurized chambers, the feel of assuming the organs like vocal cords, ears, lungs not working well, increases at high altitudes. Protocols with the Compressed Gas and Potential Risks a) Stored Compressed gas is stored in cylinder in three forms, which are storing as liquid gas, storing as compressed gas and storing as dissolved gas. In all the three forms it is much dangerous to store, as most of the stored gases are able to catch fire and as the temperature increases the pressure in the container increases and all the gas inside the container burst out and explode. In order to avoid the accidents, the gases are stored at lower temperatures and a fixed pressure is allowed to be filled into the cylinder. All gas tanks should have a tag of the compressed gas inside that shows how to maintain the safety of the compressed gas. The procedure involved in storing a gas in the tank utilizes a compressor that pushes the gas inside the tank. When a certain pressure of gas is attained, the compressor is stopped. b) Transported The compressed gas should be transported with great care to avoid any accidents. All the cylinders have to be aligned to vertical or sometimes horizontal plane in some special cases. The more appropriate method is to make horizontal beams and then the cylinders filled with the compressed gas are loaded horizontally. The openings of the cylinders can have some defects or leakages if the cylinders are placed in a wrong manner (Ridley 2011). Avoid dropping the tank of compressed gas or prevent the collision of tanks. Larger tanks have to be transported with the crt assemble separately to make risk free transportation. c) Used Compressed gas must be utilized with great care, as the compresses has high pressure, the pressurized gas will behave differently at different temperatures. In this way before utilization, the temperature of the gas must be lowered down to a stable state. It must be cared that the knob must not be opened fully, but only to half or less. Before utilizing the compressed gas, the user must check the pressure of the gas in the tank. If the pressure is more than the tagged pressure, the tank must not be used. Hospital Protocols and Dangers a) Reasons for the Difference in the Protocols The reasons for the difference in the protocols are due to enhanced safety features that are required for the hospitals. An accident would be more catastrophic when the compressed gas bursts in a closed compartment (Ridley 2011). The gas tanks should be chained separately and travelled in special tank trolleys to avoid the any accidents. Gas Laws and Hospital Equipment a) Hypobaric Chambers Hypobaric Chambers are utilized when a person experiences low pressure. In this condition, the body has low oxygen and a hypobaric chamber presents the conditions of an atmosphere, which provides an adequate amount of oxygen to the subject maintaining a certain air pressure (Rogers 2011). b) Hyperbaric Chambers When a person experiences higher pressure, hyperbaric chamber is the medicine that gradually lowers the pressure and lowers it to the atmospheric level. As the pressure reduces the absorbed gases in the blood are expelled out of the body maintaining the body in normal condition. The Henry’s law is followed to gradually lower the pressure of the container (Mathieu 2006). c) Ventilators Ventilators are essential when a person is unable to respire by himself. A ventilators works as a positive pressure ventilator (Pumps air into the lungs) or negative pressure ventilator (sucks air out of the lungs). Sometimes ventilators do both of the functions. In this way, the ventilators maintain a constant Air pressure through the lungs. The ventilators works on the principles of the gas laws. d) Oxygen Tanks Oxygen tanks are important if a patient has a breathing problem and he faces problem in inhaling. The oxygen tanks are important for the higher altitudes where the amount of oxygen in the blood reduces and causes many problems such as eye disorder (resolves when patient takes oxygen or comes to lower regions), etc. Oxygen is stored at high pressure and sometimes ina liquefied state. Obeying the gas laws. Conclusion Gas laws are important in any field of life. Boyle’s law, Charles’s law, etc are important in determining the various functions of the living beings like breathing and hearing. There is a need to develop the understanding of the gas laws. Gas laws have a variety of applications around us. In most of the industries gas laws are utilized to maintain pressure, volume and temperature. The potential risks associated with the utilization of the compressed gas can have a hazardous effects if the gas is not handled carefully. in order to maintain safety while utilizing the compressed gas, we have to follow the procedure and methods that assure safety. Never let the gas tanks to collide with the walls or with each other. Cited References Dombrink, Kathleen J., Tanis, David O. 1983. Gas Laws & Scuba Diving. Chem Matters American Chemical Society. Page 4 Holzner, Steven. 2011. Physics 1 for Dummies 2nd Edition. Wiley Publishing, New Jersey. p 307. Halliday, David, Resnick, Robert, Walker, Jearl. 2005.Halliday, Resnick and Walker’s Fundamental of Physics. Wiley Publication. p 484. Holbrow, Charles H., Lloyd, James N., Amato, Joseph C., Galvez, Enrique, Parks, M. Elizabeth. 2010. Modern Introductory Physics. Second Edition. Springer publication New York. p 89-102. Jennett, Pamela. 2004. Power Practice: Physical Sciences. Creative Teaching Press, p-31. Kotz, John C., Treichel, Paul, Townsend, John Raymond. 2009. Kotz, Treichel, Townsend Chemistry and Chemical Reactivity, Volume Two, Seventh Edition. Cengage Learning. p 524.  Kotz, John C., Treichel, Paul M., Townsend, John. 2009.Kotz, Treichel, Townsend Chemistry & Chemical Reactivity. 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