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How many moles of gas must be forced into a 4.8-L tire to

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 68P Chapter 11

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 68P

PROBLEM 68P

How many moles of gas must be forced into a 4.8-L tire to give it a gauge pressure of 32.4 psi at 25 °C? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.7 psi so that the total pressure in the tire is 47.1 psi.

Step-by-Step Solution:

Solution 68P

Here, we are going to calculate the number of moles of required gas.

Step 1:

From ideal gas equation, we have,

                                pV = nRT        ----(1)

Where, p = pressure

        V = volume of the gas

        n =  number of moles of the gas

        R =  universal gas constant and its value is 0.0821 L atm K-1 mol-1

        T =  temperature

Step 2 of 2

Chapter 11, Problem 68P is Solved
Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

The answer to “How many moles of gas must be forced into a 4.8-L tire to give it a gauge pressure of 32.4 psi at 25 °C? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.7 psi so that the total pressure in the tire is 47.1 psi.” is broken down into a number of easy to follow steps, and 50 words. This full solution covers the following key subjects: pressure, PSI, tire, Atmospheric, Gauge. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The full step-by-step solution to problem: 68P from chapter: 11 was answered by , 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 68P from 11 chapter was answered, more than 362 students have viewed the full step-by-step answer.

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