Suppose that Daniel has a 3.00 L bottle that contains a mixture of O,, N,, and CO, under a total pressure of 6.00 atm. He knows that the mixture contains 0.250 mol N, and that the partial pressure of CO, is 0.250 atm. If the temperature is 273 K, what is the partial pressure of O,? atm Po,
Suppose that Daniel has a 3.00 L bottle that contains a mixture of O,, N,, and CO, under a total pressure of 6.00 atm. He knows that the mixture contains 0.250 mol N, and that the partial pressure of CO, is 0.250 atm. If the temperature is 273 K, what is the partial pressure of O,? atm Po,
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Educational Transcription**
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**Problem Statement:**
Suppose that Daniel has a 3.00 L bottle that contains a mixture of \( O_2 \), \( N_2 \), and \( CO_2 \) under a total pressure of 6.00 atm. He knows that the mixture contains 0.250 mol \( N_2 \) and that the partial pressure of \( CO_2 \) is 0.250 atm. If the temperature is 273 K, what is the partial pressure of \( O_2 \)?
\[ P_{O_2} = \] \_\_\_\_\_ atm
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**Note:**
Students should utilize Dalton's Law of Partial Pressures to solve for the partial pressure of \( O_2 \). Dalton’s Law states that the total pressure of a gas mixture is the sum of the partial pressures of the individual gases in the mixture.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4cbada35-3122-4a6c-a25c-246bca0ae236%2F3e7f632f-726d-435d-ba49-10894e0348af%2Ffc6l5kn_processed.png&w=3840&q=75)
Transcribed Image Text:**Educational Transcription**
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**Problem Statement:**
Suppose that Daniel has a 3.00 L bottle that contains a mixture of \( O_2 \), \( N_2 \), and \( CO_2 \) under a total pressure of 6.00 atm. He knows that the mixture contains 0.250 mol \( N_2 \) and that the partial pressure of \( CO_2 \) is 0.250 atm. If the temperature is 273 K, what is the partial pressure of \( O_2 \)?
\[ P_{O_2} = \] \_\_\_\_\_ atm
---
**Note:**
Students should utilize Dalton's Law of Partial Pressures to solve for the partial pressure of \( O_2 \). Dalton’s Law states that the total pressure of a gas mixture is the sum of the partial pressures of the individual gases in the mixture.
Expert Solution
Step 1
1- First we need to determine the partial pressure of N2 :
Using ideal gas law, PV = nRT
PN2 = nRT /V
PN2 = [ 0.250mol × 0.0821atmLmol-1K-1 × 273K / 3.00L ]
PN2 = [ 5.60 / 3.00 ] atm
PN2 = 1.87 atm
Partial pressure of Nitrogen is 1.87atm
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