The atmosphere in a sealed diving bell contained oxygen and helium. If the gas mixture has 0.170 atm of oxygen and a total pressure of 3.40 atm, calculate the mass of helium in 10.5 L of the gas mixture at 17°C. Mass =
The atmosphere in a sealed diving bell contained oxygen and helium. If the gas mixture has 0.170 atm of oxygen and a total pressure of 3.40 atm, calculate the mass of helium in 10.5 L of the gas mixture at 17°C. Mass =
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...
Related questions
Question
100%
![**Problem Statement:**
The atmosphere in a sealed diving bell contained oxygen and helium. If the gas mixture has 0.170 atm of oxygen and a total pressure of 3.40 atm, calculate the mass of helium in 10.5 L of the gas mixture at 17°C.
**Calculation Required:**
Mass = _____ g
**Explanation:**
To calculate the mass of helium:
1. Use Dalton's Law of Partial Pressures to find the pressure of helium.
\[
\text{Pressure of helium} = \text{Total pressure} - \text{Pressure of oxygen} = 3.40 \, \text{atm} - 0.170 \, \text{atm}
\]
2. Use the ideal gas law to find the number of moles of helium.
\[
PV = nRT
\]
Where:
- \( P \) = pressure of helium
- \( V \) = volume (10.5 L)
- \( R \) = ideal gas constant (0.0821 L·atm/mol·K)
- \( T \) = temperature in Kelvin (add 273.15 to Celsius)
3. Calculate the mass using the molar mass of helium (4.00 g/mol).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffcaf0374-1550-4ffb-84ad-720668c0d5ec%2Fc4c91dc2-30dc-4f4a-8768-d278a33ff9c9%2Fd0odm8_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
The atmosphere in a sealed diving bell contained oxygen and helium. If the gas mixture has 0.170 atm of oxygen and a total pressure of 3.40 atm, calculate the mass of helium in 10.5 L of the gas mixture at 17°C.
**Calculation Required:**
Mass = _____ g
**Explanation:**
To calculate the mass of helium:
1. Use Dalton's Law of Partial Pressures to find the pressure of helium.
\[
\text{Pressure of helium} = \text{Total pressure} - \text{Pressure of oxygen} = 3.40 \, \text{atm} - 0.170 \, \text{atm}
\]
2. Use the ideal gas law to find the number of moles of helium.
\[
PV = nRT
\]
Where:
- \( P \) = pressure of helium
- \( V \) = volume (10.5 L)
- \( R \) = ideal gas constant (0.0821 L·atm/mol·K)
- \( T \) = temperature in Kelvin (add 273.15 to Celsius)
3. Calculate the mass using the molar mass of helium (4.00 g/mol).
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 3 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY