   # Consider the flasks in the following diagrams. a. Which is greater, the initial pressure of helium or the initial pressure of neon? How much greater? b. Assuming the connecting tube has negligible volume, draw what each diagram will look like after the stopcock between the two flasks is opened. c. Solve for the final pressure in terms of the original pressures of helium and neon. Assume temperature is constant. d. Solve for the final partial pressures of helium and neon in terms of their original pressures. Assume the temperature is constant. ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 8, Problem 82E
Textbook Problem
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## Consider the flasks in the following diagrams. a. Which is greater, the initial pressure of helium or the initial pressure of neon? How much greater?b. Assuming the connecting tube has negligible volume, draw what each diagram will look like after the stopcock between the two flasks is opened.c. Solve for the final pressure in terms of the original pressures of helium and neon. Assume temperature is constant.d. Solve for the final partial pressures of helium and neon in terms of their original pressures. Assume the temperature is constant.

a)

Interpretation Introduction

Interpretation: for the given diagram of helium and neon gases: the gas having greater pressure is to be identified with the quantity of greater pressure, the picture of diagram after the stopcock is opened is to be drawn, the final pressure in terms of original pressures of helium and neon is to be determined at constant temperature and the final partial pressures of helium and neon in terms of their original pressures are to be determined.

Concept introduction:

• At a constant volume, the pressure of gas atoms is directly proportional to number of atoms. Because more atoms means the collision will increase, so the pressure will increase.
• Partial pressure of a gas in a mixture of gases is the pressure of that gas when it alone.
• According to Boyle’s law of gas molecules,

If the volume of gases in a container is increased then the pressure will decrease at constant temperature and number of moles.

Equation for Boyle’s law is,

PinitialVinitial=PfinalVfinal

To determine: the final partial pressure of each gas in the given figure and total pressure of flask.

### Explanation of Solution

In the diagram,

There are 6 He atoms and 4 Ne atoms. The volume containing these two gases is equal. So the pressure of the gases is totally depending upon the number of molecules.

At a constant volume, the pressure of gas atoms is directly proportional to number of atoms. Because more atoms means the collision will be more, so the pressure will be more

b)

Interpretation Introduction

Interpretation: for the given diagram of helium and neon gases: the gas having greater pressure is to be identified with the quantity of greater pressure, the picture of diagram after the stopcock is opened is to be drawn, the final pressure in terms of original pressures of helium and neon is to be determined at constant temperature and the final partial pressures of helium and neon in terms of their original pressures are to be determined.

Concept introduction:

• At a constant volume, the pressure of gas atoms is directly proportional to number of atoms. Because more atoms means the collision will increase, so the pressure will increase.
• Partial pressure of a gas in a mixture of gases is the pressure of that gas when it alone.
• According to Boyle’s law of gas molecules,

If the volume of gases in a container is increased then the pressure will decrease at constant temperature and number of moles.

Equation for Boyle’s law is,

PinitialVinitial=PfinalVfinal

To determine: the final partial pressure of each gas in the given figure and total pressure of flask.

c)

Interpretation Introduction

Interpretation: for the given diagram of helium and neon gases: the gas having greater pressure is to be identified with the quantity of greater pressure, the picture of diagram after the stopcock is opened is to be drawn, the final pressure in terms of original pressures of helium and neon is to be determined at constant temperature and the final partial pressures of helium and neon in terms of their original pressures are to be determined.

Concept introduction:

• At a constant volume, the pressure of gas atoms is directly proportional to number of atoms. Because more atoms means the collision will increase, so the pressure will increase.
• Partial pressure of a gas in a mixture of gases is the pressure of that gas when it alone.
• According to Boyle’s law of gas molecules,

If the volume of gases in a container is increased then the pressure will decrease at constant temperature and number of moles.

Equation for Boyle’s law is,

PinitialVinitial=PfinalVfinal

To determine: the final partial pressure of each gas in the given figure and total pressure of flask.

d)

Interpretation Introduction

Interpretation: for the given diagram of helium and neon gases: the gas having greater pressure is to be identified with the quantity of greater pressure, the picture of diagram after the stopcock is opened is to be drawn, the final pressure in terms of original pressures of helium and neon is to be determined at constant temperature and the final partial pressures of helium and neon in terms of their original pressures are to be determined.

Concept introduction:

• At a constant volume, the pressure of gas atoms is directly proportional to number of atoms. Because more atoms means the collision will increase, so the pressure will increase.
• Partial pressure of a gas in a mixture of gases is the pressure of that gas when it alone.
• According to Boyle’s law of gas molecules,

If the volume of gases in a container is increased then the pressure will decrease at constant temperature and number of moles.

Equation for Boyle’s law is,

PinitialVinitial=PfinalVfinal

To determine: the final partial pressure of each gas in the given figure and total pressure of flask.

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