   # A collapsed balloon is filled with He to a volume of 12.5 L at a pressure of 1.00 atm. Oxygen, O 2 , is then added so that the final volume of the balloon is 26 L with a total pressure of 1.00 atm. The temperature, which remains constant throughout, is 21.5 °C. (a) What mass of He does the balloon contain? (b) What is the final partial pressure of He in the balloon? (c) What is the partial pressure of O 2 in the balloon? (d) What is the mole fraction of each gas? ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640

#### Solutions

Chapter
Section ### Chemistry & Chemical Reactivity

9th Edition
John C. Kotz + 3 others
Publisher: Cengage Learning
ISBN: 9781133949640
Chapter 10, Problem 40PS
Textbook Problem
103 views

## A collapsed balloon is filled with He to a volume of 12.5 L at a pressure of 1.00 atm. Oxygen, O2, is then added so that the final volume of the balloon is 26 L with a total pressure of 1.00 atm. The temperature, which remains constant throughout, is 21.5 °C. (a) What mass of He does the balloon contain? (b) What is the final partial pressure of He in the balloon? (c) What is the partial pressure of O2 in the balloon? (d) What is the mole fraction of each gas?

(a)

Interpretation Introduction

Interpretation:

The mass, partial pressure of He, partial pressure of O2 and mole fraction of both gas has to be given.

Concept Introduction:

• Partial pressure: The pressure of each gas in a mixture of gases is the partial pressure.
• Dalton’s law of partial pressure: The total pressure of gases in a mixture of gases is the sum of the pressure of each gas in the mixture
• Mole fraction: Quantity which defines the number of moles of a substance in a mixture divided by the total number of moles of all substances present.

xa=nantotal

pa=xa×Ptotal

Partial pressure of a gas in the mixture of gases is the product of mole fraction of the gas and the total pressure.

• Ideal gas equation:

PV=nRTP-PressureV-VolumeR-UniversalgasconstantT-Temperaturen-numberofmoles

### Explanation of Solution

The mass of helium in the balloon can be calculated as

Given:

VolumeofHe=12.5LPressure=1atmTemperature=21.5°C

According to ideal gas equation

PV=nRT

n=PVRT=1atm×12.5L0.082L.atm/K.mol×294.5K=0.517mol

Numberofmoles=massmolarmassmassofhelium

(b)

Interpretation Introduction

Interpretation:

The mass, partial pressure of He, partial pressure of O2 and mole fraction of both gas has to be given.

Concept Introduction:

• Partial pressure: The pressure of each gas in a mixture of gases is the partial pressure.
• Dalton’s law of partial pressure: The total pressure of gases in a mixture of gases is the sum of the pressure of each gas in the mixture
• Mole fraction: Quantity which defines the number of moles of a substance in a mixture divided by the total number of moles of all substances present.

xa=nantotal

pa=xa×Ptotal

Partial pressure of a gas in the mixture of gases is the product of mole fraction of the gas and the total pressure.

• Ideal gas equation:

PV=nRTP-PressureV-VolumeR-UniversalgasconstantT-Temperaturen-numberofmoles

(c)

Interpretation Introduction

Interpretation:

The mass, partial pressure of He, partial pressure of O2 and mole fraction of both gas has to be given.

Concept Introduction:

• Partial pressure: The pressure of each gas in a mixture of gases is the partial pressure.
• Dalton’s law of partial pressure: The total pressure of gases in a mixture of gases is the sum of the pressure of each gas in the mixture
• Mole fraction: Quantity which defines the number of moles of a substance in a mixture divided by the total number of moles of all substances present.

xa=nantotal

pa=xa×Ptotal

Partial pressure of a gas in the mixture of gases is the product of mole fraction of the gas and the total pressure.

• Ideal gas equation:

PV=nRTP-PressureV-VolumeR-UniversalgasconstantT-Temperaturen-numberofmoles

(d)

Interpretation Introduction

Interpretation:

The mass, partial pressure of He, partial pressure of O2 and mole fraction of both gas has to be given.

Concept Introduction:

• Partial pressure: The pressure of each gas in a mixture of gases is the partial pressure.
• Dalton’s law of partial pressure: The total pressure of gases in a mixture of gases is the sum of the pressure of each gas in the mixture
• Mole fraction: Quantity which defines the number of moles of a substance in a mixture divided by the total number of moles of all substances present.

xa=nantotal

pa=xa×Ptotal

Partial pressure of a gas in the mixture of gases is the product of mole fraction of the gas and the total pressure.

• Ideal gas equation:

PV=nRTP-PressureV-VolumeR-UniversalgasconstantT-Temperaturen-numberofmoles

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

Find more solutions based on key concepts
How do eating disorders affect health?

Understanding Nutrition (MindTap Course List)

The Dietary Guidelines for Americans recommend physical activity to help balance calorie intakes to achieve and...

Nutrition: Concepts and Controversies - Standalone book (MindTap Course List)

Provide two reasons why meiosis leads to genetic variation in diploid organisms.

Human Heredity: Principles and Issues (MindTap Course List)

How does a galactic fountain spread metals through the Galaxys disk?

Foundations of Astronomy (MindTap Course List)

Provide an example of each of the major groups of molluscs.

Oceanography: An Invitation To Marine Science, Loose-leaf Versin

One of the predicted problems due to global warming is dial ice in the polar ice caps will melt and raise sea l...

Physics for Scientists and Engineers, Technology Update (No access codes included) 