You can observe a real-life application of Boyle’s Law when you fill your bike tires with air When you pump air into a tire, the gas molecules inside the tire get compressed and packed closer together This increases the pressure of the gas, and it starts to push against the walls of the tire

Boyle was not a very social person and he never married Although, over the years, he received thousands of people into his laboratories with great hospitality, he preferred to work quietly on his own

: a statement in physics: the volume of a gas at constant temperature varies inversely with the pressure exerted on it

Real-life Examples of Boyle’s Law

• Syringe
• Human lungs
• Bicycle pump
• Coccorella atrata, a deep-sea creature
• An astronaut in outer space
• A diver in underwater
• Air bubbles on the surface of water

Why Is Boyle’s Law Important? Boyle’s law is important because it tells us about the behavior of gasses It explains, with certainty, that the pressure and volume of gas are inversely proportional to one another So, if you push on gas, its volume becomes smaller and the pressure becomes higher

Boyle’s law states the inverse relationship between pressure and volume of a gas when the temperature is held constant At an extremely high temperature the gases in question will turn to plasma Boyle’s law works, however, as long as the temperature range allows the gas to remain a gas

The volume of the gas increases as the temperature increases As temperature increases, the molecules of the gas have more kinetic energy If the container can expand, then the volume increases until the pressure returns to its original value

Another way to keep the pressure constant as the volume increases is to raise the average force that each particle exerts on the surface This happens when the temperature is increased So if the number of particles and the pressure are constant, temperature is proportional to the volume

So, that means that volume is directly proportional to temperature Even then, since we increase the temperature inside a material, the molecules’ kinetic energy increases and they start to vibrate more and move around further from each other, therefore accounting for an increase in volume

Why does a can collapse when a vacuum pump removes air from the can? The unbalanced outside force from atmospheric pressure crushes the can measured at constant temperature and pressure

Why does a can collapse when a vacuum pump removes air from the can? a The inside and outside forces balance out and crush the can The unbalanced outside force from atmospheric pressure crushes the can

A can is crushed when the pressure outside is greater than the pressure inside, and the pressure difference is greater than the can is able to withstand When the water vapor condensed, the pressure inside the can became much less than the air pressure outside Then the air outside crushed the can

The pressure outside the can is stronger and more compared to the pressure inside and hence the can pops out and collapses itself towards inside What gas law is the can crush? Crushing Can Experiment proves the Boyle’s Law, which is one of the major fundamental and experimental gas law of ideal gas equation law

The vapor from the boiling water pushed air out of the can Cooling the can caused the water vapor in the can to condense, creating a partial vacuum The extremely low pressure of the partial vacuum inside the can made it possible for the pressure of the air outside the can to crush it

When the inverted can is placed in cold water, the steam condenses, leaving the can mostly empty, and thus with a very low pressure inside of it The difference between the low pressure inside and the atmospheric pressure outside exerts an inward force on the walls of the can, causing it to implode

What this equation means is that when the air inside the can cooled, the volume decreased, causing the can to implode When the pressure inside the can decreased, the much higher air pressure outside the can pushed in the sides of the can, causing it to implode

This is, in fact, Gay-Lussac’s Law By using the heating methods, you may find that the egg is being pushed upwards by the increased air pressure inside the glass bottle Heated air rises and will escape thereby decreasing the pressure inside of the bottle

Charles’s law, a statement that the volume occupied by a fixed amount of gas is directly proportional to its absolute temperature, if the pressure remains constant

Boyle’s law—named for Robert Boyle—states that, at constant temperature, the pressure P of a gas varies inversely with its volume V, or PV = k, where k is a constant

If two letters are touching each other, they have a direct relationship That is, pressure and temperature have a direct relationship, and volume and temperature have a direct relationship That means if one of them goes up, the other will go up, assuming the third variable is held constant

We find that temperature and pressure are linearly related, and if the temperature is on the kelvin scale, then P and T are directly proportional (again, when volume and moles of gas are held constant); if the temperature on the kelvin scale increases by a certain factor, the gas pressure increases by the same factor

Boyle’s law states that the volume of a given mass of gas varies inversely with the pressure when the temperature is kept constant An inverse relationship is described in this way The k is a constant for a given sample of gas and depends only on the mass of the gas and the temperature

Boyle’s Law – states that the volume of a given amount of gas held at constant temperature varies inversely with the applied pressure when the temperature and mass are constant

Boyle’s law Because the volume has decreased, the particles will collide more frequently with the walls of the container More collisions mean more force, so the pressure will increase When the volume decreases, the pressure increases This shows that the pressure of a gas is inversely proportional to its volume