**Educational Website Content - Physics Problem** --- ### Ideal Gas Law Calculation **Problem Statement:** A sealed 11 m³ tank is filled with 5000 moles of ideal oxygen gas (diatomic) at an initial temperature of 270 K. The gas is heated to a final temperature of 380 K. The atomic mass of oxygen is 16.0 g/mol. The mass density of the oxygen gas, in SI units, is closest to: - O 18 - O 7.3 - O 29 - O 11 - O 15 --- **Explanation:** To find the mass density of the oxygen gas, we must first determine the molar mass of diatomic oxygen gas (O₂). Since each oxygen atom has an atomic mass of 16.0 g/mol, diatomic oxygen O₂ has a molar mass of: \[ \text{Molar Mass of O}_2 = 16.0 \, \text{g/mol} \times 2 = 32.0 \, \text{g/mol} \] Next, we convert this to kilograms per mole: \[ \text{Molar Mass of O}_2 = 32.0 \, \text{g/mol} = 0.032 \, \text{kg/mol} \] We can then calculate the mass of the oxygen gas using the number of moles provided: \[ \text{Mass of O}_2 = \text{number of moles} \times \text{molar mass} \] \[ \text{Mass of O}_2 = 5000 \, \text{moles} \times 0.032 \, \text{kg/mol} = 160 \, \text{kg} \] The mass density (ρ) is given by mass per unit volume: \[ \rho = \frac{\text{Mass}}{\text{Volume}} \] \[ \rho = \frac{160 \, \text{kg}}{11 \, \text{m}^3} \approx 14.5 \, \text{kg/m}^3 \] Upon rounding, the closest value is: - O 15 Therefore, **15 kg/m³** is the nearest approximation for the mass density of the oxygen gas. --- **Graphical Representation:** There are no graphs or diagrams provided with this problem
**Educational Website Content - Physics Problem** --- ### Ideal Gas Law Calculation **Problem Statement:** A sealed 11 m³ tank is filled with 5000 moles of ideal oxygen gas (diatomic) at an initial temperature of 270 K. The gas is heated to a final temperature of 380 K. The atomic mass of oxygen is 16.0 g/mol. The mass density of the oxygen gas, in SI units, is closest to: - O 18 - O 7.3 - O 29 - O 11 - O 15 --- **Explanation:** To find the mass density of the oxygen gas, we must first determine the molar mass of diatomic oxygen gas (O₂). Since each oxygen atom has an atomic mass of 16.0 g/mol, diatomic oxygen O₂ has a molar mass of: \[ \text{Molar Mass of O}_2 = 16.0 \, \text{g/mol} \times 2 = 32.0 \, \text{g/mol} \] Next, we convert this to kilograms per mole: \[ \text{Molar Mass of O}_2 = 32.0 \, \text{g/mol} = 0.032 \, \text{kg/mol} \] We can then calculate the mass of the oxygen gas using the number of moles provided: \[ \text{Mass of O}_2 = \text{number of moles} \times \text{molar mass} \] \[ \text{Mass of O}_2 = 5000 \, \text{moles} \times 0.032 \, \text{kg/mol} = 160 \, \text{kg} \] The mass density (ρ) is given by mass per unit volume: \[ \rho = \frac{\text{Mass}}{\text{Volume}} \] \[ \rho = \frac{160 \, \text{kg}}{11 \, \text{m}^3} \approx 14.5 \, \text{kg/m}^3 \] Upon rounding, the closest value is: - O 15 Therefore, **15 kg/m³** is the nearest approximation for the mass density of the oxygen gas. --- **Graphical Representation:** There are no graphs or diagrams provided with this problem
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 Website Content - Physics Problem**
---
### Ideal Gas Law Calculation
**Problem Statement:**
A sealed 11 m³ tank is filled with 5000 moles of ideal oxygen gas (diatomic) at an initial temperature of 270 K. The gas is heated to a final temperature of 380 K. The atomic mass of oxygen is 16.0 g/mol. The mass density of the oxygen gas, in SI units, is closest to:
- O 18
- O 7.3
- O 29
- O 11
- O 15
---
**Explanation:**
To find the mass density of the oxygen gas, we must first determine the molar mass of diatomic oxygen gas (O₂). Since each oxygen atom has an atomic mass of 16.0 g/mol, diatomic oxygen O₂ has a molar mass of:
\[ \text{Molar Mass of O}_2 = 16.0 \, \text{g/mol} \times 2 = 32.0 \, \text{g/mol} \]
Next, we convert this to kilograms per mole:
\[ \text{Molar Mass of O}_2 = 32.0 \, \text{g/mol} = 0.032 \, \text{kg/mol} \]
We can then calculate the mass of the oxygen gas using the number of moles provided:
\[ \text{Mass of O}_2 = \text{number of moles} \times \text{molar mass} \]
\[ \text{Mass of O}_2 = 5000 \, \text{moles} \times 0.032 \, \text{kg/mol} = 160 \, \text{kg} \]
The mass density (ρ) is given by mass per unit volume:
\[ \rho = \frac{\text{Mass}}{\text{Volume}} \]
\[ \rho = \frac{160 \, \text{kg}}{11 \, \text{m}^3} \approx 14.5 \, \text{kg/m}^3 \]
Upon rounding, the closest value is:
- O 15
Therefore, **15 kg/m³** is the nearest approximation for the mass density of the oxygen gas.
---
**Graphical Representation:**
There are no graphs or diagrams provided with this problem](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8689a897-6f19-4f8c-bce2-bc1e854b9491%2F93964256-8801-4e8e-a3b0-d59bfced077e%2F5amzx0q.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Website Content - Physics Problem**
---
### Ideal Gas Law Calculation
**Problem Statement:**
A sealed 11 m³ tank is filled with 5000 moles of ideal oxygen gas (diatomic) at an initial temperature of 270 K. The gas is heated to a final temperature of 380 K. The atomic mass of oxygen is 16.0 g/mol. The mass density of the oxygen gas, in SI units, is closest to:
- O 18
- O 7.3
- O 29
- O 11
- O 15
---
**Explanation:**
To find the mass density of the oxygen gas, we must first determine the molar mass of diatomic oxygen gas (O₂). Since each oxygen atom has an atomic mass of 16.0 g/mol, diatomic oxygen O₂ has a molar mass of:
\[ \text{Molar Mass of O}_2 = 16.0 \, \text{g/mol} \times 2 = 32.0 \, \text{g/mol} \]
Next, we convert this to kilograms per mole:
\[ \text{Molar Mass of O}_2 = 32.0 \, \text{g/mol} = 0.032 \, \text{kg/mol} \]
We can then calculate the mass of the oxygen gas using the number of moles provided:
\[ \text{Mass of O}_2 = \text{number of moles} \times \text{molar mass} \]
\[ \text{Mass of O}_2 = 5000 \, \text{moles} \times 0.032 \, \text{kg/mol} = 160 \, \text{kg} \]
The mass density (ρ) is given by mass per unit volume:
\[ \rho = \frac{\text{Mass}}{\text{Volume}} \]
\[ \rho = \frac{160 \, \text{kg}}{11 \, \text{m}^3} \approx 14.5 \, \text{kg/m}^3 \]
Upon rounding, the closest value is:
- O 15
Therefore, **15 kg/m³** is the nearest approximation for the mass density of the oxygen gas.
---
**Graphical Representation:**
There are no graphs or diagrams provided with this problem
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