Pressure-Volume Relationships in Ideal Gases

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.

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.

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

<p>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.</p> Signup and view all the answers

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

<p>$P_1V_1 = P_2V_2$</p> Signup and view all the answers

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

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

<p>$P_1V_1 = P_2V_2$</p> Signup and view all the answers

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

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

<p>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.</p> Signup and view all the answers

<p>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.</p> Signup and view all the answers

<p>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 $P_1V_1 = P_2V_2$.</p> Signup and view all the answers

<p>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.</p> Signup and view all the answers

<p>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.</p> Signup and view all the answers