   # The average lung capacity of a human is 6.0 L. How many moles of air are in your lungs when you are in the following situations? a. At sea level ( T = 298 K, P = 1.00 atm). b. 10. m below water ( T = 298 K, P = 1.97 atm). c. At the top of Mount Everest ( T = 200. K, P = 0.296 atm). ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 8, Problem 50E
Textbook Problem
2089 views

## The average lung capacity of a human is 6.0 L. How many moles of air are in your lungs when you are in the following situations?a. At sea level (T = 298 K, P = 1.00 atm).b. 10. m below water (T = 298 K, P = 1.97 atm).c. At the top of Mount Everest (T = 200. K, P = 0.296 atm).

(a)

Interpretation Introduction

Interpretation: For the given situations the number of moles of air in human lungs should be determined

Concept introduction:

By combining the three gaseous laws namely Boyle’s law, Charles’s law and Avogadro’s law a combined gaseous equation is obtained. This combined gaseous equation is called Ideal gas law.

According to ideal gas law,

PV=nRT

Where,

P = pressure in atmospheres

V= volumes in liters

n = number of moles

R =universal gas constant ( 0.08206Latm/Kmol )

T = temperature in kelvins

By knowing any three of these properties, the state of a gas can be simply identified with applying the ideal gas equation.

Number of moles of gas can be calculated from the ideal gas equation is as follows,

n=PVRT

### Explanation of Solution

According to ideal gas equation,

PV=nRT

Number of moles of gas can be calculated from the ideal gas equation is as follows,

n=PVRT ––––––––––––––––––– (1)

From the given data to calculate the number of moles, at sea level

P = 1.00atm

Since, the average capacity of human lungs is 6.0L

V = 6.0L

n =?

R =universal gas constant ( 0.08206Latm/Kmol )

(b)

Interpretation Introduction

Interpretation: For the given situations the number of moles of air in human lungs should be determined

Concept introduction:

By combining the three gaseous laws namely Boyle’s law, Charles’s law and Avogadro’s law a combined gaseous equation is obtained. This combined gaseous equation is called Ideal gas law.

According to ideal gas law,

PV=nRT

Where,

P = pressure in atmospheres

V= volumes in liters

n = number of moles

R =universal gas constant ( 0.08206Latm/Kmol )

T = temperature in kelvins

By knowing any three of these properties, the state of a gas can be simply identified with applying the ideal gas equation.

Number of moles of gas can be calculated from the ideal gas equation is as follows,

n=PVRT

(c)

Interpretation Introduction

Interpretation: For the given situations the number of moles of air in human lungs should be determined

Concept introduction:

By combining the three gaseous laws namely Boyle’s law, Charles’s law and Avogadro’s law a combined gaseous equation is obtained. This combined gaseous equation is called Ideal gas law.

According to ideal gas law,

PV=nRT

Where,

P = pressure in atmospheres

V= volumes in liters

n = number of moles

R =universal gas constant ( 0.08206Latm/Kmol )

T = temperature in kelvins

By knowing any three of these properties, the state of a gas can be simply identified with applying the ideal gas equation.

Number of moles of gas can be calculated from the ideal gas equation is as follows,

n=PVRT

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