On earth, substances tend to exist in one of three phases; either a solid, liquid, or gas. While solids and liquids have defining factors such as volume, and for solids only, a shape, gases exhibit neither of these. Gases naturally take the shape of and expand into the volume of the container, and change when placed in different surroundings. As gases are constantly moving around and colliding with the walls, they exert a force, or pressure, on the walls of its container. Pressure is one of the characteristic behaviors that gases exhibit, but due to their nature, various factor effect the pressures that a gas can exert. Towards the end of the eighteenth century, scientist began to stumble upon these various factors that affect gases, especially …show more content…
This law, known as Gay-Lussac’s law, observes the relationship between the pressure and temperature of a gas. Contrary to its name, this relationship was actually discovered by French scientific instrument inventor and physicist Guillaume Amontons, and is occasionally referred to Amontons’ Law of Pressure-Temperature. While Guy-Lussac did explore the temperature-pressure relationship, Guy-Lussac’s law is usually used to refer to the law of combining volumes. Amontons stubble across this relationship when he was building an “air thermometer.” Although not many have been able identify his exact method of experimentation, later scientist developed an apparatus in which consisted of pressure gauge and a metal sphere. These two pieces were then attached and submerged in solutions of varying temperatures. From Amontons’ and Guy-Lussac’s research and experimentation, they determined that pressure and volume had direct relationship; as one increased, the other increased. The quotient of pressure and temperature was then found to equal a constant, in which just like Boyle’s law, could be used to find one of the two variables at another pressure or temperature, given one of the variables and that the other conditions remain the same. Instead of using various solutions at different temperatures like in the experiment describe above, many experiments today utilize a solution in which the temperature is increased or decrease, such as in the following
Matter is assumed to be composed of an enormous number of very tiny particles which are indestructible. Gas is a state of matter. These tiny particles are separated by relatively large distances, which interact elastically. This large space between the particles make it easy to compress a gas. Which gives low mass to volume ratio. Particles must be in continual motion. These particles are very fast (usually about 500 meters per second). The molecules in a gaseous state have enough kinetic energy to be essentially independent of each other.
John Dalton John Dalton, born 6th September 1766, is known for developing the theory of the elements and compounds, atomic mass and weights and his research in colour blindness. He was born in Eaglesfield, Cumberland (now known as Cumbria). In school he was so successful that at the age of 12 he became a teacher. In 1785 he became one of the principles and in 1787 he made a journal that was later made into a book, describing his thoughts on mixtures of gases and how each gas acted independently and the mixtures pressure (which is the same as the gases volume if it had one). Therefore, the law of partial pressure was made.
5. In a gas increasing the pressure means molecules are more squashed up together, so there will be more collisions. My Investigation. I am going to investigate the concentration variable. I have chosen this because in my opinion it will be the easiest one to measure.
Although Black’s discovery of carbon dioxide was said to lay the foundation for modern chemistry, it wasn’t the only discovery he is credited for. He was the first to conclude that heat and temperature were two different things. Black used water as a universal substance to show that heat is energy, in which may be transported through moving and colliding molecules and the idea that temperature is the measurement of the average motion or kinetic energy of the molecules. He demonstrated this with a bucket of ice monitored by temperature constantly. The ice continually melted, but the temperature remained constant. Black is also well known for his discovery of latent heat, the heat required to convert a solid into a liquid or vapor, or a liquid into a vapor, without change of temperature. Latent heat was con be expressed in two ways: the heat can be absorbed if the change involves solid to liquid or liquid to gas or the heat can be released if the change involves gas to liquid or liquid to solid. Black took this idea and developed “specific heat”, in which is defined as the measured amount of heat required to raise the temperature of a substance by a specified number of degrees.
Laplace’s law comes from a man named Pierre-Simon Laplace, who was a French astronomer and mathematician. He was born in 1749 and died in 1827. While Laplace is known for his gas law he also studies tides and the theoretical orbits of planets and numerous other topics ("Law of laplace,”).
Robert Boyle is the most influential Anglo-Irish scientist in history. He played a key role in the history of science by establishing the experimental method, on which all modern science is based (Mollan). Also, with his assistant Robert Hooke, he began pioneering experiments on the properties of gases, including those expressed in Boyle's law. He demonstrated the physical characteristics of air, showing that is is necessary in combustion, respiration, and sound transmission. He also wrote The Sceptical Chymist in 1661, in which he attacked Aristotle's theory of four elements. This was an essential part of the modern theory of chemical elements.
Bernoulli’s principle is the concept that as the speed of a moving fluid (liquid or gas) increases, the pressure within that fluid decreases. This principle was originally formulated in 1738 by the Swiss mathematician and physicist Daniel Bernoulli, it states that the total energy in a steadily flowing ...
Vapor is the gas that forms from the vaporization of a volatile liquid. Dumas or vapor density was the method used and is done by measuring the mass of the vaporized liquid and the volume occupied by the vapor. Ideal gas law was the equation used to solve for the molecular mass of the unknown volatile sample. The purpose of this experiment is to determine the molecular mass of a substance from measurements of the density of its vapor. For the methodology, water was heated to boiling.
This law ties in with the balloon racer lab because this equation was used when trying to calculate the force and acceleration of the racer. After doing the calculations, we found that our fastest trial was in trial 3 when the racer went 0.82 m/s2 and our slowest trial was in trial 2 when the racer went 0.58 m/s2. Mass and force affected both of these results because in trial 2, we had lots of tape on the racer and condensation inside the balloon which raised the mass of the racer and caused our acceleration to be lower. After taking lots of tape off before trial 3, we noticed a huge jump in acceleration from trial 2 because now that the mass of the racer was lower. Therefore, the racer traveled at a higher acceleration in the trials after lowering the
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
Air is composed of molecules. Air is matter. It has mass and takes up space. Air is composed of different gases such as nitrogen, oxygen, carbon dioxide, water vapor, and other gases. Air molecules are in constant motion. As they move, they come in contact with surfaces. Air molecules push and press on the surfaces they contact. The amount of force per unit area that air molecules exert on a surface is called air pressure. (What is Air Pressure 6) Air pressure is caused by all of the air molecules in the Earth's atmosphere pressing down on the Earth's surfaces. We can measure air pressure to help us predict weather conditions around the world. Temperature also affects air pressure because air contracts when it cools and expands when it is heated. So if air above a region of Earth cools, it does not extend to as high an altitude as the surrounding air. In this case, its pressure at higher temperature is lower than in the surroundings even when the pressure at the surface is the same as in surrounding areas. Then air flows into the cooler region at high altitude, making the total weight of air above the region greater than in the surroundings. This is a "high". The cool air descends to the earth's surface. Near the surface, the falling air spreads out,
It is evident that pure science is the foundation of theories on which the science is built, but the application of these theories allow for a more concise understanding of the science. The application of science is not only a benefit to society in providing for many luxuries and making life less burdensome but it also helps progress science itself. Where an experiment may be able to isolate a specific variable of interest and test it, a full application provides for a complete understanding of the dynamics present in a conglomeration of forces and theories intertwined that is nature.
Gases are everywhere. Although you may not be able to see them you are surrounded by gases. Gases are in soda/pop, a hot air balloon, the tire on a bicycle and they are even in the air we breathe. There are many gases in the air we breathe. Air contains a mixture of gases including nitrogen, oxygen, argon, carbon dioxide and water vapor. Nitrogen, Oxygen, and Argon make up the greatest amount of air. Nitrogen makes up about 78% of air. Oxygen comprises approximately 21% of air. Argon constitutes 0.934%. All gases have similar physical properties. The physical properties of gases include four variables. These four variables are pressure, volume, temperature and the number of moles. These four variables can be arranged in an equation, the equation being PV=nRT. This is called the ideal gas law. One of these four variables can be figured out as long as you know the other three variables. This leads people to believe that these four variables are interdependent.
In this experiment the relationship between volume and pressure and the relationship between temperature and volume are explored with the LabQuest pressure sensor. First, the sensor and a syringe were used to find the relationship between volume and pressure by changing the volume within the syringe while it was connected to the sensor. Next the sensor was connected into an Erlenmeyer flask which was put into boiling water that was slowly lowered to 0○ to measure the change in pressure while the temperature dropped. The first relationship is called Boyle’s Law and was originally found by Robert Boyle, who published it in 16621. This law is now used to carbonate sodas. By pressurizing soda cans, the CO2 gas inside it is forced to dissolve, and when the can is opened, the pressure is relieved, and the gas begins to