General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter5: The Gaseous State
Section: Chapter Questions
Problem 5.128QP: Plot the data given in Table 5.3 for oxygen at 0C to obtain an accurate molar mass for O2. To do...
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![**Using the Ideal Gas Law to Calculate Molar Mass**
---
**Problem Statement:**
A 1.61-g sample of an unknown gas has a volume of 651 mL and a pressure of 672 mmHg at 38.8 °C. Calculate the molar mass of this compound.
**Answer Submission:**
Your answer was: **33.0 g/mol** (Incorrect).
**Options:**
- [Resubmit]
- [Show Approach]
- [Show Tutor Steps]
---
In this problem, you are required to use the Ideal Gas Law to calculate the molar mass of an unknown gas. The given parameters for the gas sample include:
- Mass (\( m \)): 1.61 g
- Volume (\( V \)): 651 mL (converted to 0.651 L for calculations)
- Pressure (\( P \)): 672 mmHg
- Temperature (\( T \)): 38.8 °C (converted to 311.95 K for calculations; remember to add 273.15 to the Celsius temperature to get Kelvin)
The Ideal Gas Law is given by:
\[ PV = nRT \]
Where:
- \( P \): pressure of the gas
- \( V \): volume of the gas
- \( n \): number of moles of gas
- \( R \): ideal gas constant (0.0821 L·atm/(K·mol) or use the appropriate value for the units given)
- \( T \): temperature in Kelvin
To find the molar mass (\( M \)), you first need to find the number of moles (\( n \)) using the equation. Note that pressure should ideally be in atmospheres (1 atm = 760 mmHg) and volume should be in liters for the standard gas constant.
Finally, molar mass is calculated using:
\[ M = \frac{m}{n} \]
In essence, this problem tests your ability to apply the Ideal Gas Law to determine the molar mass of a gas when provided with specific physical measurements.
---
**Explanation:**
This interactive problem hints at extra help options, such as:
- Showing the approach to solving
- Step-by-step guidance from a tutor
It also includes sections where you can resubmit an answer if the initial one is incorrect. For educational purposes, approaches and steps mentioned can help guide students through the systematic application of the Ideal Gas Law in practical scenarios.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffcaf0374-1550-4ffb-84ad-720668c0d5ec%2F4cb16926-50b8-4d6c-80ec-8856459d0cf4%2F132w2lc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Using the Ideal Gas Law to Calculate Molar Mass**
---
**Problem Statement:**
A 1.61-g sample of an unknown gas has a volume of 651 mL and a pressure of 672 mmHg at 38.8 °C. Calculate the molar mass of this compound.
**Answer Submission:**
Your answer was: **33.0 g/mol** (Incorrect).
**Options:**
- [Resubmit]
- [Show Approach]
- [Show Tutor Steps]
---
In this problem, you are required to use the Ideal Gas Law to calculate the molar mass of an unknown gas. The given parameters for the gas sample include:
- Mass (\( m \)): 1.61 g
- Volume (\( V \)): 651 mL (converted to 0.651 L for calculations)
- Pressure (\( P \)): 672 mmHg
- Temperature (\( T \)): 38.8 °C (converted to 311.95 K for calculations; remember to add 273.15 to the Celsius temperature to get Kelvin)
The Ideal Gas Law is given by:
\[ PV = nRT \]
Where:
- \( P \): pressure of the gas
- \( V \): volume of the gas
- \( n \): number of moles of gas
- \( R \): ideal gas constant (0.0821 L·atm/(K·mol) or use the appropriate value for the units given)
- \( T \): temperature in Kelvin
To find the molar mass (\( M \)), you first need to find the number of moles (\( n \)) using the equation. Note that pressure should ideally be in atmospheres (1 atm = 760 mmHg) and volume should be in liters for the standard gas constant.
Finally, molar mass is calculated using:
\[ M = \frac{m}{n} \]
In essence, this problem tests your ability to apply the Ideal Gas Law to determine the molar mass of a gas when provided with specific physical measurements.
---
**Explanation:**
This interactive problem hints at extra help options, such as:
- Showing the approach to solving
- Step-by-step guidance from a tutor
It also includes sections where you can resubmit an answer if the initial one is incorrect. For educational purposes, approaches and steps mentioned can help guide students through the systematic application of the Ideal Gas Law in practical scenarios.
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