Scuba Project
Allison Sadler
Gas Laws
Boyle's Law
- Relationship between pressure and volume
Charles's Law
- Volume of gas is directly related to the temperature
Dalton's Law
- Mixture of non reacting gases the total pressure exerted is equal to the sum of the partial pressures of the individual gases.
Gay- Lussac's Law
- The relationship between pressure and temperature when volume and amount are held constant.
Henry's Law
- At a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid.
The Ideal Gas Law: Crash Course Chemistry #12
"The Bends"
How do you get it?
- Occurs in scuba divers or high altitude or aerospace events when dissolved gases (mainly nitrogen) come out of solution in bubbles and can affect just about any body area including joints, lung, heart, skin and brain.
Dangers of the condition
- Life threatening and can lead to peristalsis.
Side Effects
- Fatigue and pain in muscles and joints.
How to treat the condition
- Hyperbolic decompression chamber.
Which gas?
- Henry's law because if a diver too fast, their will be too many bubbles from what was high pressure that it will cause "the bends".
USCG Medical Emergency: The Bends
Oxygen Toxicity
How do you get it?
- Breathing in molecular oxygen at increased partial pressures
Dangers of the condition
- Hypoxia and cellular and organ dysfunction or siezures
Side Effects
- Difficulty breathing and damage to the lungs
How to treat the condition
- Hyperbaric oxygen
Which gas?
- Dalton's law because the oxygen is toxic to patients of the high partial pressure.
US Navy CNS oxygen toxicity hit
Air Embolisms
How do you get it?
- Breathing in air bubbles
Dangers of the condition
- Can cause lung failure
Side Effects
- Burning sensation and coughing
How to treat the condition
- hyberberic oxygen
Which gas?
- Boyles because at lower pressures, the smaller the air bubbles will be harmful.
Air embolism (Medical Condition)