Question

What is the partial pressure of oxygen that the diver experiences at this depth?Express your answer using two significant figures. Is the diver in danger of experiencing oxygen toxicity?yesno

Answer 1

Step-by-step explanation:

Here, we know that oxygen is one of the principal component of air

As a fact, it is 21% of the total air content

What this refer to is that at any point in time, oxygen takes 0.21 the total

Mathematically, according to the Dalton's law of partialpressure, the total pressure is the sum of the individual pressure

Every constituent of the air nixture has a certain contribution in terms of the total air pressure

The partial pressure of oxygen will be the number of moles of oxygen multiplied by the total air pressure

We have this as:

`P_{O_2\text{ }}=\text{ 0.21 }*\text{ 15 = 3.2 atm}`

Finally, we want to know if the diver is in danger of experiencing air toxicity

We can get this from the limit. Whenever we have a partial pressure greater than 1.4 atm or greater, the toxicity sets in

Thus,we can be sure that the diver is in danger of air toxicity