Question

Hyperbaric therapy uses 100% oxygen at pressure to help heal wounds and infections, and to treat carbon monoxide poisoning.

Part A If the pressure inside a hyperbaric chamber is 3.0 atm, what is the volume, in liters, of the chamber containing 2300 g of O₂ at 25 °C?

Express your answer using two significant figures.

Answer 1

The volume of the hyperbaric chamber containing 2300 g of O₂ at 25 °C and 3.0 atm is approximately 5700 liters, calculated using the ideal gas law after converting the given mass to moles and the temperature to Kelvin.

Step-by-step explanation:

To calculate the volume of the hyperbaric chamber containing 2300 g of O₂ at 25 °C and 3.0 atm, we can use the ideal gas law, which states that PV = nRT, where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/K·mol), and T is the temperature in Kelvin.

First, we need to convert the mass of O₂ to moles. Oxygen has a molar mass of 32.00 g/mol, so:

n = mass / molar mass = 2300 g / 32.00 g/mol = 71.875 moles of O₂

Next, convert the temperature to Kelvin:

T = 25 °C + 273.15 = 298.15 K

Now, insert the values into the ideal gas law equation:

PV = nRT

V = nRT / P = (71.875 mol) * (0.0821 L·atm/K·mol) * (298.15 K) / 3.0 atm

V ≈ 5745.77 L

Therefore, the volume of the hyperbaric chamber is approximately 5745.77 liters, which we can express using two significant figures as 5700 liters.