Question

A scuba diver 40 ft below the ocean surface inhales 800 mL of compressed air from a scuba tank at a pressure of 3.50 atm and a temperature of 9°C You may want to reference (Pogon 209 - 200) Section 8 5 while completing this problem Part A What is the pressure of the itin atm, in the lungs when the gas expands to 1800 mL at a body temperature of 37 "Cand the amount of gas remains constant? Express the pressure in atmospheren to throw nignificant riguroa. ΠΡΟ ΑΣφ P. at

Answer 1

The scuba diver's expanded gas pressure in the lungs, at a volume of 1800 mL and body temperature of 37 degrees Celsius, is 4.09 atm. This is calculated using Gay-Lussac's Law.

Step-by-step explanation:

The situation is an example of the gas law. This law states that the pressure and volume of a gas have an inverse relationship when temperature is held constant. We can apply Gay-Lussac's Law here, which states that the pressure of a gas is directly proportional to its absolute temperature if the volume is kept constant. First, we need to convert the temperatures to the Kelvin scale. After that, we can set up the equation (P1/T1 = P2/T2) where P1 is the initial pressure, T1 is the initial temperature, P2 is the final pressure, and T2 is the final temperature.

To calculate this, let's convert the celsius temperatures to Kelvin. 9 degrees celsius is 282.15 K and 37 degrees celsius is 310.15 K. Plugging the values into the equation we have, (3.5 atm / 282.15 K) = P2 / 310.15 K. Solving for P2 gives us 4.09 atm as the pressure of the expanded gas in the scuba diver's lungs.

Learn more about Gas Laws