Uses and Applications of the Different Gas Laws

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Juan Sumulong Memorial Junior College School Year 2009-2010 Taytay, Rizal

Chemistry Project

Submitted by: Dan Paolo Petalbo Submitted to: Mr. Rufino Panganiban Jr.

Boyle’s Law Uses/Applications 1)

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Many gases are stored under high pressure. This way they would occupy a smaller volume. This is an application of Boyle’s Law. For example, some cars use compressed natural gas as fuel. The mechanics of a bicycle pump is governed by Boyle’s Law. The washer in a bicycle pump allows air enters the barrel from outside during the upstroke, but during the down stroke, this air can no longer escape to the outside and is compressed in the barrel. As the volume decreases, the pressure increases, but at first, the air cannot escape because the valve in the bicycle inner tube prevents it from entering that tube. This valve is closed because the pressure of the air already in the tube prevents the entry of further gas. Only when the pressure of the air in the pump is greater than that in the inner tube will the valve open and allow more air into the tube, further increasing the pressure. This means that, at the next stroke of the pump, the air will have to be compressed even more. As the pressure in the tube increases, it gets harder and harder to depress the pump. Suppose that you buy a bag of chips at the top of a mountain, once you hit the bottom of the mountain, the bag explodes, causing chips to fly everywhere. This is because the air contained in the bag expanded as the pressure inside of the bag increased. A practical application illustrating Boyles Law would be the action of a syringe. When we draw fluids into a syringe, we increase the volume inside the syringe, this correspondingly decreases the pressure on the inside where the pressure on the outside of the syringe is greater and forces fluid into the syringe. If we reverse the acting and push the plunger in on the syringe we are decreasing the volume on the inside which will increase the pressure inside making the pressure greater than on the outside and fluids are forced out.

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A more life dependent example of Boyles Law is the action of the diaphragm of our body. This is a muscle that is located just below the lungs. When we inhale the diaphragm moves downward allowing the lungs an increased volume. This decreases the pressure inside the lungs so that the pressure is less than the outer pressure. This results in forcing air into the lungs. When we exhale the diaphragm moves upward and decreases the volume of the lungs. This increases the pressure inside the lungs above the pressure on the outside of the lungs so that gases are forced out of the lungs. Of course, all of this is totally automatic and we take this important cycle which is performed hundreds of times a day for granted until we receive a sharp blow to that region that briefly paralyzes the diaphragm muscle. We say the wind was knocked out of us, but Boyles Law was not allowed to function. Fish that live in low depths survive under a great amount of pressure due to the volume of water above them. When brought to the surface of the ocean, perhaps for study, the dramatically reduced pressure greatly increases the volume of the gases in their bodies. This causes the rupture of cells, bladders, and other biological structures. While playing in the pool when you were younger, did you ever notice that when you exhaled, the bubbles seemed to grow larger and larger as they ascended? This change in size is a result of the decreasing pressure of the water, which allows the gas bubbles to expand.

Charles’s Law Uses/Applications 1)

When flying hot-air balloons, balloonists apply the principle of Charles’s Law. As the air inside the balloon is heated, its volume increases. The density of the air decreases as the air inside the balloon is heated; it expands, resulting in an increase in density of the air inside the balloon. The density of hot air is less than of cold air. The difference in density between the air inside and outside the balloon makes the hot-air balloon rise.

2) Weather balloons are launched daily from weather stations across the country. The balloon begins at the earth at a certain P, T, and V and upon its accent all three of these variables change in response to the surroundings. 3) A rubber raft swells up when left in the sun on a hot day, providing the raft is not completely inflated (if it completely inflated, it will rupture). Remember this if you are ever stranded in tropical waters! 5) The plunger in a turkey thermometer pops out when the turkey is done. The higher temperature of the turkey causes the volume of the air trapped under the plunger to increase, which forces the plunger to move.

Combined Gas Law Uses/Applications 1)

A four stroke engine like your car operates on the principle of taking a volume of gas/air mixture, compressing it, igniting it, and pushing the exhaust out. The movement of the pistons moves the drive shaft.

Ideal Gas Law Uses/Applications 1)

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Commercial airlines pressurize their passenger cabins and mountain climbers often carry oxygen tanks with them. The air at these higher altitudes is at lower atmospheric pressure or is ``thinner.'' This phenomenon in which pressure decreases with increasing altitude occurs in all fluids (liquids and gases) and is particularly pronounced when water is the fluid. On the ocean floor the water pressure can be enormous! This is why submarines and other deep sea diving vessels must have thick walls to prevent them from being crushed under tremendous water pressures.

Dalton’s Law of Partial Pressure

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A common laboratory method of collecting the gaseous product of a chemical reaction is to conduct it into an inverted tube or bottle filled with water, the opening of which is immersed in a larger container of water. This arrangement is called a pneumatic trough, and was widely used in the early days of chemistry. As the gas enters the bottle it displaces the water and becomes trapped in the upper part. The volume of the gas can be observed by means of a calibrated scale on the bottle, but what about its pressure? The total pressure confining the gas is just that of the atmosphere transmitting its force through the water. (An exact calculation would also have to take into account the height of the water column in the inverted tube.) But liquid water itself is always in equilibrium with its vapor, so the space in the top of the tube is a mixture of two gases: the gas being collected, and gaseous H2O. The partial pressure of H2O is known as the vapor pressure of water and it depends on the temperature. In order to determine the quantity of gas we have collected, we must use Dalton's Law to find the partial pressure of that gas.