Answered

Scuba divers use compressed air to breathe while underwater.
When filled with compressed air, a typical scuba tank with a volume of 13.2 L has a
pressure of 153 atm at a temperature of 37 °C. If the water temperature is 3.0 °C, how
many liters of air (when out of the tank) will such a tank provide to a diver's lungs at a
depth of approximately
in the ocean where the pressure is ?
L
Enter the value with the appropriate number of significant figures.



Answer :

andrewrodriguez1130
Hey Andrew! To calculate the volume of air a scuba tank will provide to a diver's lungs at a certain depth, we can use the combined gas law, which states: (P1 * V1) / (T1) = (P2 * V2) / (T2), where:
- P1, V1, and T1 are the initial pressure, volume, and temperature of the air in the tank.
- P2 is the pressure at the depth where the diver is, V2 is the volume of air the diver breathes, and T2 is the temperature at that depth.

Given:
- P1 = 153 atm
- V1 = 13.2 L
- T1 = 37 °C (which is 310 K)
- T2 = 3.0 °C (which is 276 K)
- P2 is the pressure at the depth where the diver is, which you didn't specify.

We can solve for V2 (the volume of air the diver breathes) using the formula. Let me know the pressure at the depth where the diver is, and I can help you calculate the volume of air the tank will provide to the diver's lungs.