PADI PADI Physics & Physiology of Diving

Question 1

Which gas law explains why a full scuba tank will show a lower pressure reading on a cold day compared to a warm day?

Accepted Answer

Charles's Law

Answer

Boyle's Law

Answer

Dalton's Law

Answer

Henry's Law

Question 2

According to Boyle's Law, what happens to the volume of an air space as a diver descends to greater depth?

Accepted Answer

It decreases proportionally as pressure increases

Answer

It stays the same

Answer

It increases with depth

Answer

It doubles every 33 feet

Question 3

What is 'nitrogen narcosis' and at what approximate depth does it typically begin to affect recreational divers?

Accepted Answer

An intoxicating effect of nitrogen under pressure, often noticeable around 100 feet (30 m)

Answer

Nitrogen bubbles forming in the blood, occurring below 60 feet

Answer

A toxic reaction to oxygen at depths below 40 feet

Answer

Nitrogen depletion causing fatigue at any depth

Question 4

What physiological condition results from ascending too quickly and allowing dissolved nitrogen to form bubbles in body tissues?

Accepted Answer

Decompression Sickness (DCS)

Answer

Oxygen Toxicity

Answer

Hypercapnia

Answer

Squeeze

Question 5

What does Dalton's Law of Partial Pressures state in the context of scuba diving?

Accepted Answer

The total pressure of a gas mixture equals the sum of the partial pressures of each component gas

Answer

Gas volume decreases as pressure increases

Answer

Temperature and gas pressure are proportional

Answer

Gas dissolves in liquid proportionally to its partial pressure

Question 6

At 2 atmospheres of pressure (33 feet/10 meters), what happens to the volume of a diver's lungs if they hold their breath and ascend to the surface?

Accepted Answer

The volume doubles, risking lung overexpansion injury

Answer

The volume stays the same

Answer

The volume halves

Answer

The volume increases by 50%