Question

Using real world examples, describe how changes in temperature, volume and pressures effect the behavior of a gas according to the following laws: Boyle's Law, Charles' Law, and Gay-Lussac's Law.

Answer 1

Boyle's Law, Charles's Law, and Gay-Lussac's Law describe the relationship between pressure, volume, and temperature in gases. Examples include the use of syringes (Boyle's Law), the functioning of hot air balloons (Charles's Law), and the behavior of aerosol cans in heat (Gay-Lussac's Law). Temperatures must be expressed in Kelvins for accurate predictions.

Step-by-step explanation:

Understanding Gas Laws

The behavior of gases can be understood through different gas laws that describe how temperature, volume, and pressure affect a gas. These laws are important for explaining real-world phenomena such as breathing, cooking, and even weather forecasting.

Boyle's Law

Boyle's Law states that the pressure of a gas is inversely proportional to its volume when the temperature and the number of moles of the gas are held constant. A real-world example of Boyle's Law is the functioning of a syringe. When you pull the plunger up, the volume inside the barrel increases, leading to a decrease in pressure, which in turn draws liquid into the syringe.

Charles's Law

Charles's Law explains that a gas's volume is directly proportional to its temperature (measured in Kelvins) at constant pressure and amount. Hot air balloons are a practical application of Charles's Law. As the air inside the balloon is heated, it expands and hence it occupies more volume, causing the balloon to rise due to the reduction in air density inside it.

Gay-Lussac's Law

Gay-Lussac's Law describes how the pressure of a gas is directly proportional to its absolute temperature at constant volume and amount of gas. An example of this can be seen in a closed aerosol can. If the can is heated, the pressure inside the can increases as the temperature of the gas increases, which could potentially lead to the can bursting.

In all gas laws, temperatures must be expressed in Kelvin to ensure accuracy in calculations and predictions. These laws provide crucial insights into the behavior of gases in various conditions, and they are applied in a multitude of scientific and engineering disciplines.

Answer 2

There are three laws that explain the behaviour of ideal gases:

1) Boyle's law:

"For a constant mass of ideal gas kept at constant temperature, the pressure of the gas is inversely proportional to the gas volume"

Mathematically:

`p\propto (1)/(V)`

where

p is the pressure of the gas

V is its volume

An example of application of Boyle's law is in the gas inside a syringe: if we block the nozzle of the syringe, and we push on the other side, we compress the volume of the gas inside; as a result, we notice that it becomes more and more difficult to push the other side of the syringe: this is because the pressure of the gas inside is increasing, due to Boyle's law.

2) Charle's Law:

"For a constant mass of an ideal gas kept at constant pressure, the volume of the gas is proportional to its absolute temperature"

Mathematically:

`V\propto T`

where

V is the volume of the gas

T is its absolute temperature (in Kelvin)

An easy example of application of Charle's law is a helium balloon. If we fill a balloon with helium gas, then we bring the ballon to another place with lower temperature, we notice that the balloon shrinks: this is because the temperature of the gas has decreased, and therefore the volume of the balloon decreases as well. Vice-versa, if we bring the balloon to a warmer place, it expands: the temperature has increased, and therefore the volume increases as well.

3) Gay-Lussac's law:

"For a constant mass of an ideal gas kept at constant volume, the pressure of the gas is proportional to its absolute temperature"

Mathematically:

`p\propto T`

where

p is the pressure of the gas

T is the absolute temperature of the gas (in Kelvin)

An example of Gay-Lussac's law in daily life is a canister containing gas. The canister has a fixed volume, so does the gas inside. If the canister is placed above a flame, heat is transferred to the gas inside the canister: as result, the temperature of the gas increases. According to Gay-Lussac's law, the pressure increases as well: therefore, at some point, the pressure of the gas will be large enough to break the canister, which will then explode.