A 6.00L tank C is filled with 4.09g of cabron monoxide gas and 4.36g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits.
A 6.00L tank C is filled with 4.09g of cabron monoxide gas and 4.36g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits.
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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A 6.00L tank C is filled with 4.09g of cabron monoxide gas and 4.36g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions.
Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits.
![### Problem Statement
A 6.00 L tank at 6.72 °C is filled with 4.09 g of carbon monoxide gas and 4.36 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions.
### Task
Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits.
### Data Table
| **Gas** | **Mole Fraction** | **Partial Pressure (atm)** |
|-----------------------------|------------------|---------------------------|
| **Carbon Monoxide (CO)** | | |
| **Dinitrogen Difluoride (N2F2)** | | |
| **Total Pressure in Tank** | | |
### Interactive Component
There is an interactive tool next to the data table indicating possible numeric inputs. Users may enter their answers using the input boxes and verify them.
### Explanation
To calculate the mole fraction and partial pressure for each gas, follow these steps:
1. **Molecular Weight Calculation**:
- Calculate the molecular weight of each gas (CO and N2F2).
2. **Mole Calculation**:
- Compute the number of moles for each gas using the formula:
\[
\text{Moles} = \frac{\text{Mass}}{\text{Molecular Weight}}
\]
3. **Total Moles Calculation**:
- Add up the moles of both gases to get the total moles.
4. **Mole Fraction Calculation**:
- The mole fraction of each gas is the ratio of moles of that gas to the total moles:
\[
\text{Mole Fraction} = \frac{\text{Moles of Gas}}{\text{Total Moles}}
\]
5. **Partial Pressure Calculation**:
- Use the Ideal Gas Law \( PV = nRT \) to calculate the total pressure in the tank.
- \( P \): Total pressure
- \( V \): Volume (6.00 L)
- \( n \): Total moles (sum of moles of CO and N2F2)
- \( R \): Ideal Gas Constant (0.0821 L·atm·K⁻¹·mol⁻¹)
- \( T \): Temperature in](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9757754f-3312-4a82-9461-9956fc98753f%2Fcebc92c6-9063-4ce4-afd2-2b9d87508bce%2F16pt413_processed.png&w=3840&q=75)
Transcribed Image Text:### Problem Statement
A 6.00 L tank at 6.72 °C is filled with 4.09 g of carbon monoxide gas and 4.36 g of dinitrogen difluoride gas. You can assume both gases behave as ideal gases under these conditions.
### Task
Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits.
### Data Table
| **Gas** | **Mole Fraction** | **Partial Pressure (atm)** |
|-----------------------------|------------------|---------------------------|
| **Carbon Monoxide (CO)** | | |
| **Dinitrogen Difluoride (N2F2)** | | |
| **Total Pressure in Tank** | | |
### Interactive Component
There is an interactive tool next to the data table indicating possible numeric inputs. Users may enter their answers using the input boxes and verify them.
### Explanation
To calculate the mole fraction and partial pressure for each gas, follow these steps:
1. **Molecular Weight Calculation**:
- Calculate the molecular weight of each gas (CO and N2F2).
2. **Mole Calculation**:
- Compute the number of moles for each gas using the formula:
\[
\text{Moles} = \frac{\text{Mass}}{\text{Molecular Weight}}
\]
3. **Total Moles Calculation**:
- Add up the moles of both gases to get the total moles.
4. **Mole Fraction Calculation**:
- The mole fraction of each gas is the ratio of moles of that gas to the total moles:
\[
\text{Mole Fraction} = \frac{\text{Moles of Gas}}{\text{Total Moles}}
\]
5. **Partial Pressure Calculation**:
- Use the Ideal Gas Law \( PV = nRT \) to calculate the total pressure in the tank.
- \( P \): Total pressure
- \( V \): Volume (6.00 L)
- \( n \): Total moles (sum of moles of CO and N2F2)
- \( R \): Ideal Gas Constant (0.0821 L·atm·K⁻¹·mol⁻¹)
- \( T \): Temperature in
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