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# A scuba diver breathing normal air descends to 100 m of ## Problem 82P Chapter 11

Introductory Chemistry | 5th Edition

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Problem 82P

PROBLEM 82P

A scuba diver breathing normal air descends to 100 m of depth, where the total pressure is 11 atm. What is the partial pressure of oxygen that the diver experiences at this depth? Is the diver in danger of experiencing oxygen toxicity?

Step-by-Step Solution:

Solution 82P

Here, we are going to calculate the partial pressure of oxygen that the diver experiences at this depth.

Step 1:

Given that, the scuba diver is breathing normal. So the percentage of oxygen in air is 21% which is fixed.

Partial pressure of a component can be calculated by using the following formula.

Partial Pressure of a component : x Total pressure

Step 2:

Partial Pressure of a Oxygen : x 11 atm = 2.31 atm

The partial pressure of oxygen that the diver experiences at this depth is 2.31 atm.

Step 3 of 3

##### ISBN: 9780321910295

This full solution covers the following key subjects: diver, oxygen, pressure, depth, experiencing. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. Introductory Chemistry was written by Patricia and is associated to the ISBN: 9780321910295. The answer to “A scuba diver breathing normal air descends to 100 m of depth, where the total pressure is 11 atm. What is the partial pressure of oxygen that the diver experiences at this depth? Is the diver in danger of experiencing oxygen toxicity?” is broken down into a number of easy to follow steps, and 42 words. The full step-by-step solution to problem: 82P from chapter: 11 was answered by Patricia, our top Chemistry solution expert on 05/06/17, 06:45PM. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. Since the solution to 82P from 11 chapter was answered, more than 973 students have viewed the full step-by-step answer.

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