Aim • The experiment has three objectives: • Validation of the Boyle’s gas law • Determination of the gas moles used in the experiment • Establishing the Universal Gas Constant (R) Introduction / Background Gases take one form of physical appearance for substances. By definition, a gas represents a grouping of molecules at a high energy such that the volume it occupies is determined by container, and can be molded and compressed into smaller packages via reduction of energy. Manipulating energy is the gases results into a change in form and physical appearance, which engages various phases from solid, liquid and gas. In the gaseous form the pressure (P), volume (V), absolute temperature of the gas (T), molar gas constant (R) and the number of moles (n) are the factors that can be manipulated to derive various characteristics of the gas to establish a relationship between the characteristic of the gas (Castka, Metcalfe, Davis, & Williams, 2002). The traits of a gas in its ideal form are governed by the relationship: PV = n RT (Guch, 2003). A change in either of the values in the relationship results in a change to the other variable of the gas. Assessing the behavior of gases via manipulation of the characteristics is done by holding the factors constant (Zumdahl, 1998). Where the number of gas moles, molar gas constant, and volume of the gas remain constant, a change in the temperature of the gas results to a change in the pressure as well. The ideal relationship between the gas factors is quite complex to be evaluated since it involves holding three of the five factors constant while two factors are assessed. Different gas laws derived from the ideal gas law can be evaluated individually since control can be easier conducted in l... ... middle of paper ... ...oth values of P obtained. • There was no temperature change; else, it would not have remained constant failing to validate Boyle’s law. • Converting the pressures into absolutes was not necessary in calculating R. Summary/ Conclusion The experiment validated the relationship between pressure and volume, thus proves Boyle’s law. The universal gas constant that was obtained was lower than the theoretical value, which could have been attributed to errors in the experiment. References Castka, J. F., Metcalfe, H. C., Davis, R. E., & Williams, J. E. (2002). Modern Chemistry. New York: Holt, Rinehart and Winston. Guch, I. (2003). The Complete Idiot's Guide to Chemistry. New York: Alpha, Penguin Group Inc. Meyer, S. (2011). Gases and Their Properties. New York: The Rosen Publishing Group. Zumdahl, S. S. (1998). Chemical Principles. New York: Houghton Mifflin Company.
It was learned that changing the volume of the same substance will never change the boiling point of the substance. However having two different substances with the same volume will result in two different boiling points. The purpose of this lab was to determine if changing the volume of a substance will change the boiling point. This is useful to know in real life because if someone wanted to boil water to make pasta and did not know how much water to
middle of paper ... ... The Web. 22 Feb. 2014. http://www.chemheritage.org/discover/online-resources/chemistry-in-history>.
We thank the University of Oklahoma and the chemistry faculty for providing the space, instructions, and equipment for the development of this report and experiment.
3. Corey, E. J., Barbara Czako, and Laszlo Kurti. Molecules and medicine. New Jersey: John
The molar mass of butane gas (C4H10)can be obtained theoretically by using a periodic table, but by rearranging the ideal gas law equation (PV = nRT) to n =PVRT, the experimental molar mass of butane gas can be found. In the equation, P= pressure in atmosphere, V= volume in liters, n= moles, R= 0.0821, and T= temperature in kelvin. To find the values for the equation, the mass of the butane released from a pressurized container and the volume of that gas will be found, and the method of water displacement at room conditions will be used to find the rest of the values. Then, the molar mass will
Sootin, Harry, and Gustav Schrotter.Robert Boyle : founder of modern chemistry. New York: F. Watts, 1962. Print.
Gas Laws: Avogadro’s Law: equivalent volumes of gases under same temperatures and pressured conditions will have equivalent number of atoms (particles, molecules, ions, electrons, etc). Charles’ Law: as temperature increases the volume of the gas increases too (directly proportional) providing that the pressure and the amount of gas is constant Boyle’s Law: as pressure of the gas increases the volume decreases. As volume increases, the pressure of the gas decreases. Temperature is constant. Guy-Lussac’s Law: as temperature of the gas increases the pressure of the gas increases as well provided that the volume and the amount of gas are constant.
Boston: Unwin Hyman, 1988. Works Consulted -. Sazlberg, Hugh W. From Caveman to Chemist: Circumstances and Achievements. Washington, D.C.: American Chemical Society, 1991.
Chemistry is critical to resolving today’s problems. Each day's news contains concerns where chemistry matters, everything from quicker and affordable drug development, cleaner and more efficient fuel sources, safer air and purified drinking water, the design of faster computers and molecular machines, biotechnology to develop fitness and food sources across the globe, nanotechnology to reduce the size and ecological impact of many consumer goods, and green industrial procedures to limit pollution. Recent technical innovations and enrichments have undoubtedly added immensely to the applications of chemistry. So, I ask myself, why not chemistry? I see chemistry as the answer to the question of human’s survival, the hope of better days to come, careers to be established, and influences to be
Next Dalton’s law of partial pressure is used. The mixture of gas in the graduated cylinder was filled with two things: water vapor and air. Using the Dalton’s law, it can be concluded that the total pressure is equal to the pressure of air and the pressure of water vapor added together. This is an endothermic reaction which means that it absorbs heat, and when a reaction gains heat, it is repres...
Bruce Mattson. “Henry Cavendish 1731-1810”. History of Gas Chemistry. Updated September 25, 2001. Retrieved December 1, 2011
Since the days of Aristotle, all substances have been classified into one of three physical states. A substance having a fixed volume and shape is a solid. A substance, which has a fixed volume but not a fixed shape, is a liquid; liquids assume the shape of their container but do not necessarily fill it. A substance having neither a fixed shape nor a fixed volume is a gas; gases assume both the shape and the volume of their container. The structures of gases, and their behavior, are simpler than the structures and behavior of the two condensed phases, the solids and the liquids
Plontke, R. (2003, March 13). Chemnitz UT. TU Chemnitz: - Technische Universität Chemnitz. Retrieved April 1, 2014, from http://www.tu-chemnitz.de/en/
Physics is the branch of science, which deals with the motion, and the causes of the motion on a specific body. However, what causes this motion? The answer is forces that are in action. This subject of motion under forces is termed as Mechanics. Every object around us shows some type of motion, for example Sun and the other planets are going in circular motion and many other examples are all undergoing in the action of some kind of forces. The motion of fluids or liquids under the action of some forces is termed as fluid mechanics. Fluids may include any type of liquids, gasses, or plasma. The study of these phases and their motion is very important and they have been widely used in many modern life applications.
Despite wide differences in chemical properties, all the gases, more or less on a grand scale, obey “the gas laws”. The gas laws deal with how the behavior of gases varies with changes in pressure, temperature, volume, and number of particles (moles as we call it in class). The first law is Boyle’s Law, which is the pressure-volume law. In terms of each other, the pressure-volume law states that “the volume of a given amount of gas held at constant temperature varies inversely with the applied pressure when temperature and mass are constant”. Another way to identify it, is by saying that their products are constant