Pressure-Volume Relationships in Ideal Gases

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What is Boyle's Law and what does it state?

Boyle's Law states that as long as the temperature is held constant, the pressure and volume of a gas are inversely proportional to each other. Meaning, if one increases, the other one decreases.

What does Boyle's law state?

Boyle's law states that for an ideal gas held at a constant temperature, the product of the pressure and volume must be constant, showing an inverse relationship between pressure and volume.

What are the two factors used in Boyle's law?

The two factors used in Boyle's law are pressure and volume.

Give an example of a real-life application of Boyle's law.

An example of a real-life application of Boyle's law is breathing. When the lungs change volume, this creates a difference in pressure inside the body relative to the atmosphere, driving air in and out of the lungs. Signup and view all the answers

What does Boyle's Law state?

Boyle's Law states that the pressure and volume of a gas are inversely proportional to each other, assuming the temperature is constant. Signup and view all the answers

How can Boyle's Law be expressed in equation form?

$P_1V_1 = P_2V_2$ Signup and view all the answers

If a container filled with an ideal gas at 2 atm occupies 2L of space, and the volume is doubled to 4L, what is the pressure inside the container?

The pressure inside the container would decrease to 1 atm. Signup and view all the answers

According to Boyle's Law, what is the relationship between the pressure and volume of a gas?

The pressure and volume of a gas are inversely proportional to each other. Signup and view all the answers

What is the equation that represents Boyle's Law?

$P_1V_1 = P_2V_2$ Signup and view all the answers

If a balloon at sea level with a volume of 1 liter experiences a decrease in pressure to 0.5 atmospheres, what will be the final volume of the balloon?

The final volume of the balloon will be 2 liters. Signup and view all the answers

According to Boyle's law, what is the relationship between the pressure and volume of an ideal gas?

The relationship between the pressure and volume of an ideal gas is inverse. When the pressure increases, the volume decreases and vice versa. Signup and view all the answers

How does Boyle's law explain the relationship between volume and pressure in a gas?

Boyle's law states that the product of the pressure and volume of an ideal gas is constant. This means that if the volume of a gas is reduced, the pressure increases, and if the volume is increased, the pressure decreases. Signup and view all the answers

How does Boyle's law relate to the behavior of gases in the human body?

Boyle's law explains how the lungs function during breathing. When the muscles in the body pull on the lungs, increasing their volume, the pressure in the lungs decreases below atmospheric pressure, causing air to be forced into the lungs. When the lungs contract, decreasing their volume, the pressure inside increases, forcing air back out. Signup and view all the answers

According to Boyle's law, what is the relationship between pressure and volume of an ideal gas at a constant temperature?

The relationship between pressure and volume of an ideal gas at a constant temperature is inversely proportional. If the pressure of the system increases, the volume must decrease, and vice versa. This relationship can be described using the equation $P_1V_1 = P_2V_2$. Signup and view all the answers

If the original pressure of a gas system is 1.2 atm and the final pressure is 2.4 atm after the volume has been adjusted, what was the initial volume of the gas?

To find the initial volume, we can use Boyle's law equation $P_1V_1 = P_2V_2$. Given that $P_1 = 1.2$ atm, $P_2 = 2.4$ atm, and $V_2 = 22.0$ L, we can solve for $V_1$. Rearranging the equation, we have $V_1 = \frac{{P_2V_2}}{{P_1}} = \frac{{2.4 , \text{atm} \times 22.0 , \text{L}}}{{1.2 , \text{atm}}} \approx 44.0$ L. Signup and view all the answers

Johnny's air-filled scuba vest holds 1.43 liters of air at 1.03 atmospheres of pressure. What volume of air will it hold at 10 meters underwater, which is equivalent to about 2.03 atmospheres?

Using Boyle's law equation $P_1V_1 = P_2V_2$, we can solve for the final volume $V_2$. Given that $P_1 = 1.03$ atm, $V_1 = 1.43$ L, and $P_2 = 2.03$ atm, we can rearrange the equation to solve for $V_2$. We have $V_2 = \frac{{P_1V_1}}{{P_2}} = \frac{{1.03 , \text{atm} \times 1.43 , \text{L}}}{{2.03 , \text{atm}}} \approx 0.726$ L. Signup and view all the answers

Pressure-Volume Relationships in Ideal Gases

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