If the gas mixture in Question #13 above has a temperature of 37°C and a volume of 52.0 L: a. What is the mass of the nitrogen gas in the mixture? b. What is the mass of the oxygen gas in the mixture? c. What is the mass of the helium gas in the mixture? d. What is the mass of the carbon dioxide gas in the mixture? e. What is the total mass of the all the gas in the mixture?
If the gas mixture in Question #13 above has a temperature of 37°C and a volume of 52.0 L: a. What is the mass of the nitrogen gas in the mixture? b. What is the mass of the oxygen gas in the mixture? c. What is the mass of the helium gas in the mixture? d. What is the mass of the carbon dioxide gas in the mixture? e. What is the total mass of the all the gas in the mixture?
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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The first picture has the atm numbers from question 13
Transcribed Image Text:### Gas Mixture Questions for Educational Purposes
#### Given Conditions:
- Temperature: 37°C
- Volume: 52.0 L
#### Questions:
a. What is the mass of the nitrogen gas in the mixture?
b. What is the mass of the oxygen gas in the mixture?
c. What is the mass of the helium gas in the mixture?
d. What is the mass of the carbon dioxide gas in the mixture?
e. What is the total mass of all the gas in the mixture?
![### Calculating Partial Pressures of Gases
This tutorial explains how to calculate the partial pressures of different gases from a total pressure using given percentages. Here are the step-by-step calculations:
#### (a) Calculating the Partial Pressure of \( N_2 \)
Given:
- Total pressure, \(P_{\text{total}} = 3039.750 \text{kPa}\)
- Percentage of \( N_2 \) in the mixture = \( 47.28\% \)
**Formula:**
\[P_{N_2} = P_{\text{total}} \times \left(\frac{47.28}{100}\right)\]
\[
\begin{aligned}
P_{N_2} &= 3039.750 \text{kPa} \times \left(\frac{47.28}{100}\right) \\
&= 1437.2 \text{kPa} \\
&= 1437.2 \times 0.00987 \text{ atm} \\
&= 14.2 \text{ atm}
\end{aligned}
\]
#### (b) Calculating the Partial Pressure of \( O_2 \)
Given:
- Percentage of \( O_2 \) in the mixture = \( 17.92\% \)
**Formula:**
\[P_{O_2} = P_{\text{total}} \times \left(\frac{17.92}{100}\right)\]
\[
\begin{aligned}
P_{O_2} &= 3039.750 \text{kPa} \times \left(\frac{17.92}{100}\right) \\
&= 544.72 \text{kPa} \\
&= 544.72 \times 0.00987 \text{ atm} \\
&= 5.38 \text{ atm}
\end{aligned}
\]
#### (c) Calculating the Partial Pressure of \( He \)
Given:
- Percentage of \( He \) in the mixture = \( 29.77\% \)
**Formula:**
\[P_{He} = P_{\text{total}} \times \left(\frac{29.77}{100}\right)\]
\[
\begin{aligned}
P_{He} &= 3039.750 \text{kPa} \times \left(\frac{29.77}{100}\](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fec9904e6-dc28-47e5-ba82-a0b2892d5fea%2F3f2840be-9697-44f2-badf-5d78020b2f6d%2Fykgujab_processed.png&w=3840&q=75)
Transcribed Image Text:### Calculating Partial Pressures of Gases
This tutorial explains how to calculate the partial pressures of different gases from a total pressure using given percentages. Here are the step-by-step calculations:
#### (a) Calculating the Partial Pressure of \( N_2 \)
Given:
- Total pressure, \(P_{\text{total}} = 3039.750 \text{kPa}\)
- Percentage of \( N_2 \) in the mixture = \( 47.28\% \)
**Formula:**
\[P_{N_2} = P_{\text{total}} \times \left(\frac{47.28}{100}\right)\]
\[
\begin{aligned}
P_{N_2} &= 3039.750 \text{kPa} \times \left(\frac{47.28}{100}\right) \\
&= 1437.2 \text{kPa} \\
&= 1437.2 \times 0.00987 \text{ atm} \\
&= 14.2 \text{ atm}
\end{aligned}
\]
#### (b) Calculating the Partial Pressure of \( O_2 \)
Given:
- Percentage of \( O_2 \) in the mixture = \( 17.92\% \)
**Formula:**
\[P_{O_2} = P_{\text{total}} \times \left(\frac{17.92}{100}\right)\]
\[
\begin{aligned}
P_{O_2} &= 3039.750 \text{kPa} \times \left(\frac{17.92}{100}\right) \\
&= 544.72 \text{kPa} \\
&= 544.72 \times 0.00987 \text{ atm} \\
&= 5.38 \text{ atm}
\end{aligned}
\]
#### (c) Calculating the Partial Pressure of \( He \)
Given:
- Percentage of \( He \) in the mixture = \( 29.77\% \)
**Formula:**
\[P_{He} = P_{\text{total}} \times \left(\frac{29.77}{100}\right)\]
\[
\begin{aligned}
P_{He} &= 3039.750 \text{kPa} \times \left(\frac{29.77}{100}\
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