Boyle's Law and Universal Gas Constant (Coursework Sample)

Boyle’s Law and Universal Gas Constant
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Boyle’s Law and Universal Gas Constant
The Boyle’s law is one of the gas laws that were developed towards the end of 18th century. . It specifically describes the relationship between the volume of an ideal gas and its absolute pressure within a closed system. The temperature and mass of the gas must be kept constant for the law to hold. According to Susan (2011), the law states that at constant temperature and fixed mass, the absolute pressure of a gas is inversely proportional to its volume. This is to mean that when one quantity doubles, the other one halves. The mathematical expression of Boyle’s law is PV=constant or P1V1=P2V2, where P is the pressure of the system, V is the volume of the gas, and K is the constant of that particular gas.
Boyle’s law applies only to an ideal gas. For real gases, when they are compressed at a constant temperature, changes in the relationship between the volume and pressure occur. The law is however accurate enough to be used in a number of practical real life applications. All types of syringes use Boyle’s law to operate. When you pull the plunger out on a syringe, it makes the volume of the chamber to increase, creating a vacuum. When the volume increases it makes the pressure to reduce. Any fluid that is available on the other side of the syringe is sucked into the chamber as a result of attempt to balance the pressure within the chamber of the syringe with the atmospheric pressure. Also when you shake a soda bottle the carbon dioxide gas in the can mixes with the soda making the cap to pop off. The reason for this is that the gas is able to increase in volume making the pressure within the bottle more. As the bubbles try to muscle their way out, they push the soda along with it.
The universal gas constant also known as the ideal gas constant is a physical constant that appears in the thermo-chemical equations defining the behavior of gases under theoretical ideal conditions. Conventionally, the universal gas constant is symbolized R and it has a value of 8.3144621J/K.mol. The pressure, amount of substance (mole), volume, and temperature of a gas are all related according to the equation PV=nRT. Form this equation, the value of the molar gas constant R= PV/nR. In this equation, P represents pressure, V the volume, n the amo...