Final answer:
The question regarding the volume of oxygen supplied by a hyperbaric oxygen chamber at a given pressure cannot be answered definitively without additional information about the new pressure. If the oxygen is assumed to be released to 1 atm, using Boyle's Law, the volume would be 120.0 L.
Step-by-step explanation:
The volume of oxygen supplied by a hyperbaric oxygen chamber from a pressurized cylinder can be calculated using the gas laws, specifically Boyle's Law, if temperature is constant. For the cylinder holding 30.0 L of oxygen at 4.0 atm, the question appears to ask what the volume would be at a different pressure. However, no new pressure is provided, so we must assume the question is asking for the initial volume, which is already given as 30.0 L. It may also be possible that the question implies the volume of oxygen when it is released to 1 atm pressure, as commonly done in medical applications.
Using the gas law: P₁V₁ = P₂V₂, where P means pressure and V means volume, a simple calculation can be made if a new pressure is given. For example, if the oxygen is released to 1 atm, the new volume V₂ can be calculated by rearranging the formula to V₂ = (P₁V₁)/P₂. Plugging in the numbers, V₂ = (4.0 atm * 30.0 L) / 1 atm = 120.0 L, so the cylinder would supply 120.0 L under those conditions. If a different pressure is required for the calculation, then the final volume would change accordingly.