Chapter U3.60, Problem 7E

(a)

Interpretation Introduction

Interpretation:

The information regarding the variation in pressure from $\text{1 atm}$ to $\text{3}\text{.5 atm}$ at sea level and inside sea is given. The effect of pressure change from $\text{1 atm}$ to $\text{3}\text{.5 atm}$ over volume of lungs has to be explained.

Concept Introduction :

Boyle’s law is used to describe the relation between volume and pressure.

Answer to Problem 7E

The volume of lungs will decrease on change of pressure from $\text{1 atm}$ to $\text{3}\text{.5 atm}$ .

Explanation of Solution

According to Boyle’s law at the conditions of constant temperature and constant number of particles, the relationship between pressure and volume of gas is given as shown below.

  $PV=\text{constant}$

Thus, both pressure and volume are inversely proportional to each other. Now, when the pressure increases to $\text{3}\text{.5 atm}$ then volume being inversely proportional will decrease. Thus, volume of lungs will be less at $\text{3}\text{.5 atm}$ than at a pressure of 1 atm.

(b)

Interpretation Introduction

Interpretation:

The reason for danger involved in holding breath and ascending quickly has to be explained.

Concept Introduction :

Boyle’s law is used to describe the relation between volume and pressure.

Answer to Problem 7E

Holding breathe and ascending quickly may lead to the rupture of the lungs due to sudden change in pressure.

Explanation of Solution

The pressure of air keeps on increasing on going deep down in the sea. Now pressure inside the sea is very high while it is low at the sea level. Now if the person tries to ascend above by holding breathe then the rupture of lungs may occur. This may happen because outside pressure is decreasing on moving up while the pressure inside the lungs is same and is higher than upward pressure. Thus, if the person will go up directly then it will affect the lungs. Therefore, it is advised to slowly release breathe while ascending towards the sea level.