A woman has an initial long volume of 2.7 L which is filled with air atm pressure of 1.02 at the moment if she increases her lung volume 3.2 L just by using her equations muscles within without inhaling any additional air what is the new pressure in her lungs

Question

Which Law would you use to solve this problem? (1 point) Responses Charles' Law Charles' Law Boyle's Law Boyle's Law Combined Gas Law Combined Gas Law Ideal Gas Law

Answer 1

To solve this problem, you would use Boyle's Law.

Boyle’s Law states that the pressure of a gas is inversely proportional to its volume when the temperature and the amount of gas are held constant. The formula is given by:

\[ P_1 \times V_1 = P_2 \times V_2 \]

Where:

• \( P_1 \) is the initial pressure,
• \( V_1 \) is the initial volume,
• \( P_2 \) is the final pressure, and
• \( V_2 \) is the final volume.

In this case:

• \( P_1 = 1.02 , \text{atm} \)
• \( V_1 = 2.7 , \text{L} \)
• \( V_2 = 3.2 , \text{L} \)

You can rearrange the equation to solve for \( P_2 \):

\[ P_2 = \frac{P_1 \times V_1}{V_2} \]

Now you can substitute the values:

\[ P_2 = \frac{1.02 , \text{atm} \times 2.7 , \text{L}}{3.2 , \text{L}} \]

Calculating this gives:

\[ P_2 = \frac{2.754 , \text{atm \cdot L}}{3.2 , \text{L}} \] \[ P_2 \approx 0.859375 , \text{atm} \]

So the new pressure in her lungs when she increases the volume to 3.2 L is approximately 0.86 atm.