The ratio of helium to oxygen must be used if the diver is at an ocean depth of 50.0 m.

Question

Want to see the full answer?

Answer 1

Question

Chapter 21, Problem 53AP

To determine

The ratio of helium to oxygen must be used if the diver is at an ocean depth of 50.0 m.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

You have completed several dives using SCUBA apparatus and are ready for a deep dive in seawater. You have arranged to have tanks of heliox prepared for your dive. Heliox is a mixture of helium and oxygen. Oxygen at pressures much greater than 1 atm is toxic to lung cells, so you want to keep the partial pressure of oxygen from your diving equipment at 1 atm or less during your dive. You will be diving at a depth of h = 41.8 m. What ratio of helium to oxygen, by weight, should you request for the mixtures in your tanks? The partial pressure of a gas in a mixture is the pressure the gas would have if it existed by itself in the same volume. Dalton's law of partial pressures tells us that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases. (The density of seawater is 1,030 kg/m³. Assume the air pressure at sea level is 1 atm.) WHe = 0.77 Wo2 Find the ratio of numbers of molecules for the two gases first, demanding that the oxygen…

You have completed several dives using SCUBA apparatus and are ready for a deep dive in seawater. You have arranged to have tanks of heliox prepared for your dive. Heliox is a mixture of helium and oxygen. Oxygen at pressures much greater than 1 atm is toxic to lung cells, so you want to keep the partial pressure of oxygen from your diving equipment at 1 atm or less during your dive. You will be diving at a depth of h = 51.8 m. What ratio of helium to oxygen, by weight, should you request for the mixtures in your tanks? The partial pressure of a gas in a mixture is the pressure the gas would have if it existed by itself in the same volume. Dalton's law of partial pressures tells us that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the individual gases. (The density of seawater is 1,030 kg/m³. Assume the air pressure at sea level is 1 atm.) WHE W02

A deep-sea diver should breathe a gas mixture that has the same oxygen partial pressure as at sea level, where dry air contains 20.9% oxygen and has a total pressure of 1.01 X 105 N/m2. (a) What is the partial pressure of oxygen at sea level? (b) If the diver breathes a gas mixture at a pressure of 2.00 X 106 N/m2, what percent oxygen should it be to have the same oxygen partial pressure as at sea level?