Aerosol cans and gas laws
Global issue- During World War II the U.S government supported an investigation into finding a portable way for service men to spray malaria carrying bugs. Finding cure for malaria was a massive issue all over the world during World War 2 but when the cure was found the only possible way to prevent the disease from spreading was by killing the malarial bugs through spraying them. Getting a portable can to spray them was a huge problem during the World War 2 era as there was no design of spray cans that could be used when the disease was an outbreak at this time. Malaria was very infectious and deadly as there was not yet a way to kill the malaria carrying bugs.
There remains much need for innovative methods to …show more content…
These collisions apply a pressure per unit area and cause the gases to occupy a volume. The "head space" of an aerosol can is filled with extremely pressurized propellant found in a gas form and goes with Henry's law as an equivalent quantity of this propellant is deliquesced in the product itself. As soon as the nozzle gets depressed, the pressure of the propellant forces the product out through the nozzle. Both the pressure and volume are affected by temperature and the relationship between these three variables was expressed by Boyle, Charles, and Gay-Lussac and can be applied to pharmaceutical aerosols or aerosol cans. Boyle’s law is a gas law that relates the volume of a gas to the pressure since through this the pressure formed by a static mass of gas increases as the volume decreases and the gas is held at a constant temperature which shows that pressure is inversely proportional to the …show more content…
Even though the P, V and T of each condition may be different, the ratio is constant and expressed as:PV/T=R in which R us the constant value of the ratio. This equation is made considering only 1 mole [like one gram molecular weight] of ideal gas. If n moles of a gas were to be considered then it would be PV=nRT which is known as the general ideal gas law. R will be the molar gas constant and can be used in many different units depending on the application:8.314 J/K/mole, 0.08205 L atm/mole and 1.987mole. The relevance of the gas laws to aerosol cans can be seen in the following
Global issue- During World War II the U.S government supported an investigation into finding a portable way for service men to spray malaria carrying bugs. Finding cure for malaria was a massive issue all over the world during World War 2 but when the cure was found the only possible way to prevent the disease from spreading was by killing the malarial bugs through spraying them. Getting a portable can to spray them was a huge problem during the World War 2 era as there was no design of spray cans that could be used when the disease was an outbreak at this time. Malaria was very infectious and deadly as there was not yet a way to kill the malaria carrying bugs.
There remains much need for innovative methods to …show more content…
These collisions apply a pressure per unit area and cause the gases to occupy a volume. The "head space" of an aerosol can is filled with extremely pressurized propellant found in a gas form and goes with Henry's law as an equivalent quantity of this propellant is deliquesced in the product itself. As soon as the nozzle gets depressed, the pressure of the propellant forces the product out through the nozzle. Both the pressure and volume are affected by temperature and the relationship between these three variables was expressed by Boyle, Charles, and Gay-Lussac and can be applied to pharmaceutical aerosols or aerosol cans. Boyle’s law is a gas law that relates the volume of a gas to the pressure since through this the pressure formed by a static mass of gas increases as the volume decreases and the gas is held at a constant temperature which shows that pressure is inversely proportional to the …show more content…
Even though the P, V and T of each condition may be different, the ratio is constant and expressed as:PV/T=R in which R us the constant value of the ratio. This equation is made considering only 1 mole [like one gram molecular weight] of ideal gas. If n moles of a gas were to be considered then it would be PV=nRT which is known as the general ideal gas law. R will be the molar gas constant and can be used in many different units depending on the application:8.314 J/K/mole, 0.08205 L atm/mole and 1.987mole. The relevance of the gas laws to aerosol cans can be seen in the following