Chapter 5.8, Problem 5.7CC

(a)

Interpretation Introduction

Interpretation:

A $\text{1}\text{.00 L}$ container is filled with ideal gas, then the same amount of real gas is put into the same container.

When the real gas molecules occupy a relatively small volume and have large intermolecular attractions, the pressure of the two gases has to be compared.

Concept Introduction:

Ideal Gas Law:

The ideal gas equation is:

$\text{PV = nRT}$

Where,

P is the pressure

V is the volume

T is the temperature

R is molar gas constant

n is the mole

(b)

Interpretation Introduction

Interpretation:

A $\text{1}\text{.00 L}$ container is filled with ideal gas, then the same amount of real gas is put into the same container.

When the real gas molecules occupy a relatively large volume and have negligible intermolecular attractions, the pressure of the two gases has to be compared.

Concept Introduction:

Ideal Gas Law:

The ideal gas equation is:

$\text{PV = nRT}$

Where,

P is the pressure

V is the volume

T is the temperature

R is molar gas constant

n is the mole

(c)

Interpretation Introduction

Interpretation:

A $\text{1}\text{.00 L}$ container is filled with ideal gas, then the same amount of real gas is put into the same container.

When the real gas molecules occupy a relatively large volume and have large intermolecular attractions, the pressure of the two gases has to be compared.

Concept Introduction:

Ideal Gas Law:

The ideal gas equation is:

$\text{PV = nRT}$

Where,

P is the pressure

V is the volume

T is the temperature

R is molar gas constant

n is the mole