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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sorry for the bad photo, but #6 is the one I need help with
![**Educational Content:**
---
**Section 5:**
- A 256-mL flask containing air has a mass of 119.2861 g. If the mass of the flask filled with water is 378.26 g, what is the volume of air in the flask? (Density of water = 0.9975 g/mL)
**Solution Steps:**
\[
\text{Mass of water} = 378.26 \text{ g} - 119.2861 \text{ g} = 258.9739 \text{ g}
\]
Using the density of water:
\[
\text{Volume of water} = \frac{258.9739 \text{ g}}{0.9975 \text{ g/mL}} = 259.6 \text{ mL}
\]
**Section 6:**
- What is the volume of a gas at standard conditions (STP) if the volume at 1.014 atm and 286.7 K is 246.7 mL?
**Conditions:**
\[
\text{Initial Pressure} = 1.014 \text{ atm}
\]
\[
\text{Initial Temperature} = 286.7 \text{ K}
\]
\[
\text{Initial Volume} = 246.7 \text{ mL}
\]
Using the ideal gas law or relevant formulas, calculate the volume at STP, integrating changes in pressure and temperature.
**Section 7:**
- Assuming natural gas is entirely methane (CH₄), what would the density be at standard conditions?
\[
\text{Molar mass of methane} = 16.04 \text{ g/mol}
\]
Further calculations would involve using the ideal gas law for density determination at standard conditions.
---
**Note:** Ensure all calculations are cross-verified for accuracy and comprehensiveness in educational scenarios. Use this template for educational purposes and not as a final definitive calculation without proper validation from scientific practices.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3831c069-cf0d-4055-80ae-ed1ea5fcd99d%2F2c4272c6-ddfb-4991-9976-7f8530dae0f1%2Fwneuiff_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Content:**
---
**Section 5:**
- A 256-mL flask containing air has a mass of 119.2861 g. If the mass of the flask filled with water is 378.26 g, what is the volume of air in the flask? (Density of water = 0.9975 g/mL)
**Solution Steps:**
\[
\text{Mass of water} = 378.26 \text{ g} - 119.2861 \text{ g} = 258.9739 \text{ g}
\]
Using the density of water:
\[
\text{Volume of water} = \frac{258.9739 \text{ g}}{0.9975 \text{ g/mL}} = 259.6 \text{ mL}
\]
**Section 6:**
- What is the volume of a gas at standard conditions (STP) if the volume at 1.014 atm and 286.7 K is 246.7 mL?
**Conditions:**
\[
\text{Initial Pressure} = 1.014 \text{ atm}
\]
\[
\text{Initial Temperature} = 286.7 \text{ K}
\]
\[
\text{Initial Volume} = 246.7 \text{ mL}
\]
Using the ideal gas law or relevant formulas, calculate the volume at STP, integrating changes in pressure and temperature.
**Section 7:**
- Assuming natural gas is entirely methane (CH₄), what would the density be at standard conditions?
\[
\text{Molar mass of methane} = 16.04 \text{ g/mol}
\]
Further calculations would involve using the ideal gas law for density determination at standard conditions.
---
**Note:** Ensure all calculations are cross-verified for accuracy and comprehensiveness in educational scenarios. Use this template for educational purposes and not as a final definitive calculation without proper validation from scientific practices.
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