If you pump air into a tire, you're increasing the pressure, and the tire expans. Which means when presure is increased, so is the volume. Isn't this a violation of Boyle's Law?
Boyle's Law simply describes the relationship between the pressure and volume of an enclosed gas when Temperature remains constant. That relationship, usually expressed as P1 V1 = P2 V2, just means that the product of pressure x volume remains unchanged as either or both are changed.
Since pressure x volume remains constant, for example, doubling the pressure on an enclosed gas will reduce its volume to 1/2 its previous size. Tripling the pressure will reduce its volume to 1/3, and so on. Alternatively, if you double the volume available to an enclosed gas, pressure is halved.
Boyle's Law is a hand bicycle pump. By pushing down on the piston, the volume of the gas decreases, the molecules are now having more chances of collisions with the interior walls of the pump and this increases the pressure of the air inside so that it is forced into the tire.
The relationship between pressure and volume is called Boyle's Law. Boyle's Law also says that volume is inversely proportional to pressure. That means that if the volume of a gas goes up the pressure goes down and if the volume of the gas goes up the pressure goes down. The air pressure inside of an inflated balloon is more than the atmospheric pressure outside the balloon. Also, the density inside the balloon is greater than the density outside. The molecules inside the balloon move around and bang against the inner walls. Their impacts on the inner walls produce a force, which provides the pressure of the enclosed air. Because of Boyle's Law if you squeeze a balloon to halve its volume you end up increasing the pressure on the balloon. Also pressure is directly proportional to density. That means, if the pressure in the balloon increases, so does the density, and if the pressure goes down then the density decreases also. Because of that, when you squeeze the balloon and halve its volume you increase the density of the balloon. The increase in pressure that occurs when you halve the volume of the balloon is why balloons pop when you squeeze them.
Boyle's Law simply describes the relationship between the pressure and volume of an enclosed gas when Temperature remains constant. That relationship, usually expressed as P1 V1 = P2 V2, just means that the product of pressure x volume remains unchanged as either or both are changed.
Since pressure x volume remains constant, for example, doubling the pressure on an enclosed gas will reduce its volume to 1/2 its previous size. Tripling the pressure will reduce its volume to 1/3, and so on. Alternatively, if you double the volume available to an enclosed gas, pressure is halved.
Boyle's Law is a hand bicycle pump. By pushing down on the piston, the volume of the gas decreases, the molecules are now having more chances of collisions with the interior walls of the pump and this increases the pressure of the air inside so that it is forced into the tire.
The relationship between pressure and volume is called Boyle's Law. Boyle's Law also says that volume is inversely proportional to pressure. That means that if the volume of a gas goes up the pressure goes down and if the volume of the gas goes up the pressure goes down. The air pressure inside of an inflated balloon is more than the atmospheric pressure outside the balloon. Also, the density inside the balloon is greater than the density outside. The molecules inside the balloon move around and bang against the inner walls. Their impacts on the inner walls produce a force, which provides the pressure of the enclosed air. Because of Boyle's Law if you squeeze a balloon to halve its volume you end up increasing the pressure on the balloon. Also pressure is directly proportional to density. That means, if the pressure in the balloon increases, so does the density, and if the pressure goes down then the density decreases also. Because of that, when you squeeze the balloon and halve its volume you increase the density of the balloon. The increase in pressure that occurs when you halve the volume of the balloon is why balloons pop when you squeeze them.
