Part A Three gases (8.00 g of methane, CH4, 18.0 g of ethane, CH6, and an unknown amount of propane, C3Hs) were added to the same 10.0-L container. At 23.0 °C, the total pressure in the container is 3.60 atm . Calculate the partial pressure of each gas in the container. Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane. • View Available Hint(s) ? atm Part B A gaseous mixture of O2 and N2 contains 40.8 % nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 545 mmHg ? Express you answer numerically in millimeters of mercury. • View Available Hint(s) Poxygen mmHg
Part A Three gases (8.00 g of methane, CH4, 18.0 g of ethane, CH6, and an unknown amount of propane, C3Hs) were added to the same 10.0-L container. At 23.0 °C, the total pressure in the container is 3.60 atm . Calculate the partial pressure of each gas in the container. Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane. • View Available Hint(s) ? atm Part B A gaseous mixture of O2 and N2 contains 40.8 % nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 545 mmHg ? Express you answer numerically in millimeters of mercury. • View Available Hint(s) Poxygen mmHg
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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Please answer question 9 Part A and B
![Dalton's law states that the total pressure, \( P_{\text{total}} \), of a mixture of gases in a container equals the sum of the pressures of each individual gas:
\[ P_{\text{total}} = P_1 + P_2 + P_3 + \ldots \]
The partial pressure of the first component, \( P_1 \), is equal to the mole fraction of this component, \( X_1 \), times the total pressure of the mixture:
\[ P_1 = X_1 \times P_{\text{total}} \]
The mole fraction, \( X \), represents the concentration of the component in the gas mixture, so:
\[ X_1 = \frac{\text{moles of component 1}}{\text{total moles in mixture}} \]
### Part A
Three gases (8.00 g of methane, \( \text{CH}_4 \), 18.0 g of ethane, \( \text{C}_2\text{H}_6 \), and an unknown amount of propane, \( \text{C}_3\text{H}_8 \)) were added to the same 10.0-L container. At 23.0 °C, the total pressure in the container is 3.60 atm. Calculate the partial pressure of each gas in the container.
**Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane.**
\[ \_\_\_\_\_ \text{ atm} \]
### Part B
A gaseous mixture of \( \text{O}_2 \) and \( \text{N}_2 \) contains 40.8% nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 545 mmHg?
**Express your answer numerically in millimeters of mercury.**
\[ P_{\text{oxygen}} = \_\_\_\_\_ \text{ mmHg} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fded90a0e-1aa2-42d3-8902-387fb21746ad%2Fac7fa96a-38a1-4260-a9e8-681d250e84ac%2F75uht8k_processed.png&w=3840&q=75)
Transcribed Image Text:Dalton's law states that the total pressure, \( P_{\text{total}} \), of a mixture of gases in a container equals the sum of the pressures of each individual gas:
\[ P_{\text{total}} = P_1 + P_2 + P_3 + \ldots \]
The partial pressure of the first component, \( P_1 \), is equal to the mole fraction of this component, \( X_1 \), times the total pressure of the mixture:
\[ P_1 = X_1 \times P_{\text{total}} \]
The mole fraction, \( X \), represents the concentration of the component in the gas mixture, so:
\[ X_1 = \frac{\text{moles of component 1}}{\text{total moles in mixture}} \]
### Part A
Three gases (8.00 g of methane, \( \text{CH}_4 \), 18.0 g of ethane, \( \text{C}_2\text{H}_6 \), and an unknown amount of propane, \( \text{C}_3\text{H}_8 \)) were added to the same 10.0-L container. At 23.0 °C, the total pressure in the container is 3.60 atm. Calculate the partial pressure of each gas in the container.
**Express the pressure values numerically in atmospheres, separated by commas. Enter the partial pressure of methane first, then ethane, then propane.**
\[ \_\_\_\_\_ \text{ atm} \]
### Part B
A gaseous mixture of \( \text{O}_2 \) and \( \text{N}_2 \) contains 40.8% nitrogen by mass. What is the partial pressure of oxygen in the mixture if the total pressure is 545 mmHg?
**Express your answer numerically in millimeters of mercury.**
\[ P_{\text{oxygen}} = \_\_\_\_\_ \text{ mmHg} \]
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