An open flask sitting in a lab refrigerator looks empty, but it is actually filled with a mixture of gases called air. If the flask volume is 4.50 L, and the air is at standard temperature and pressure, how many gaseous molecules does the flask contain? number of gaseous molecules:
An open flask sitting in a lab refrigerator looks empty, but it is actually filled with a mixture of gases called air. If the flask volume is 4.50 L, and the air is at standard temperature and pressure, how many gaseous molecules does the flask contain? number of gaseous molecules:
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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Question 8
![**Understanding the Number of Gaseous Molecules in a Flask**
An interesting phenomenon in the study of gases is that an open flask sitting in a lab refrigerator may appear empty, but it is, in fact, filled with a mixture of gases known as air. To explore this further, consider the following scenario:
**Problem Statement:**
If the flask volume is 4.50 liters (L), and the air is at standard temperature and pressure (STP), how many gaseous molecules does the flask contain?
**Calculation Section:**
To find the number of gaseous molecules, apply the Ideal Gas Law and Avogadro's principle. At STP (0°C and 1 atm), one mole of any gas occupies 22.4 L, and contains Avogadro's number of molecules (\(6.022 \times 10^{23}\) molecules/mol).
**Number of Gaseous Molecules:**
- Calculate the number of moles of gas in the flask:
\[
\text{Moles of gas} = \frac{\text{Flask volume (L)}}{\text{Volume of 1 mole at STP (L/mol)}} = \frac{4.50 \, \text{L}}{22.4 \, \text{L/mol}} \approx 0.201 \, \text{mol}
\]
- Calculate the number of molecules:
\[
\text{Number of molecules} = \text{Moles of gas} \times \text{Avogadro's number} = 0.201 \, \text{mol} \times 6.022 \times 10^{23} \, \text{molecules/mol}
\]
Plug in the values to get the final count and insert the value in the box provided:
**Number of Gaseous Molecules:** [_______]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe4db1e84-75df-498d-9686-5cabfd0e0c2f%2F809a42ef-502d-4cc4-a265-02dfe4b9a430%2Fdk7xza_processed.png&w=3840&q=75)
Transcribed Image Text:**Understanding the Number of Gaseous Molecules in a Flask**
An interesting phenomenon in the study of gases is that an open flask sitting in a lab refrigerator may appear empty, but it is, in fact, filled with a mixture of gases known as air. To explore this further, consider the following scenario:
**Problem Statement:**
If the flask volume is 4.50 liters (L), and the air is at standard temperature and pressure (STP), how many gaseous molecules does the flask contain?
**Calculation Section:**
To find the number of gaseous molecules, apply the Ideal Gas Law and Avogadro's principle. At STP (0°C and 1 atm), one mole of any gas occupies 22.4 L, and contains Avogadro's number of molecules (\(6.022 \times 10^{23}\) molecules/mol).
**Number of Gaseous Molecules:**
- Calculate the number of moles of gas in the flask:
\[
\text{Moles of gas} = \frac{\text{Flask volume (L)}}{\text{Volume of 1 mole at STP (L/mol)}} = \frac{4.50 \, \text{L}}{22.4 \, \text{L/mol}} \approx 0.201 \, \text{mol}
\]
- Calculate the number of molecules:
\[
\text{Number of molecules} = \text{Moles of gas} \times \text{Avogadro's number} = 0.201 \, \text{mol} \times 6.022 \times 10^{23} \, \text{molecules/mol}
\]
Plug in the values to get the final count and insert the value in the box provided:
**Number of Gaseous Molecules:** [_______]
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