Question

31. Hyperbaric therapy uses 100% oxygen at pressure to help heal wounds and infections, and to treat carbon monoxide poisoning. A hyperbaric chamber has a volume of 1510 L. How many kilograms of O2 gas are needed to give an oxygen pressure of 2.04 atm at 25 °C?

Answer 1

To determine the number of kilograms of O2 gas needed for a specific oxygen pressure in a hyperbaric chamber, we can use the ideal gas law equation:

PV = nRT

Where:
P = pressure (in atm)
V = volume (in L)
n = number of moles of gas
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)

First, let's convert the temperature from Celsius to Kelvin:
25 °C + 273.15 = 298.15 K

Now, we can rearrange the ideal gas law equation to solve for the number of moles of gas (n):
n = PV / RT

Plugging in the given values:
P = 2.04 atm
V = 1510 L
R = 0.0821 L·atm/(mol·K)
T = 298.15 K

n = (2.04 atm * 1510 L) / (0.0821 L·atm/(mol·K) * 298.15 K)

Now, we can convert the number of moles of gas to kilograms using the molar mass of oxygen (O2):
Molar mass of O2 = 32 g/mol

n (in mol) * Molar mass of O2 (in g/mol) = mass of O2 (in g)

Finally, we can convert the mass of O2 from grams to kilograms:
mass of O2 (in g) / 1000 = mass of O2 (in kg)

I hope this helps! Let me know if you have any further questions.