Chapter 5, Problem 88E

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,

  ${\text{P}}_{\text{initial}}{\text{V}}_{\text{initial}}\text{=}{\text{P}}_{\text{final}}{\text{V}}_{\text{final}}$

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

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,

  ${\text{P}}_{\text{initial}}{\text{V}}_{\text{initial}}\text{=}{\text{P}}_{\text{final}}{\text{V}}_{\text{final}}$

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,

  ${\text{P}}_{\text{initial}}{\text{V}}_{\text{initial}}\text{=}{\text{P}}_{\text{final}}{\text{V}}_{\text{final}}$

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,

  ${\text{P}}_{\text{initial}}{\text{V}}_{\text{initial}}\text{=}{\text{P}}_{\text{final}}{\text{V}}_{\text{final}}$

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