Chapter 5, Problem 131AE

a)

Interpretation Introduction

Interpretation: The qualitative graphs that distinguish between the following properties have to be drawn.

PV versus V at constant T

Concept Introduction

Ideal gas law: This law expressed by following equation is,

$\text{PV = nRT}$

Where,

$\begin{array}{l}\text{P - Pressure}\\ \text{V - volume}\\ \text{n - Number of moles}\\ \text{R - Gasconstant}\\ \text{T -Temperature}\end{array}$

Boyle’s law: Boyle’s law states that relationship between pressure of the gas and volume. That is pressure is inversely proportional to volume.

$\text{Pressure}\text{α}\frac{\text{1}}{\text{Volume}}$

Charles’s law: This law states that relationship between volume of an ideal gas and temperature at constant pressure. That is volume is directly proportional to temperature.

$\text{Volume α Temperature}$

b)

Interpretation Introduction

Interpretation: The qualitative graphs that distinguish between the following properties have to be drawn.

P versus T at constant V

Concept Introduction

Ideal gas law: This law expressed by following equation is,

$\text{PV = nRT}$

Where,

$\begin{array}{l}\text{P - Pressure}\\ \text{V - volume}\\ \text{n - Number of moles}\\ \text{R - Gasconstant}\\ \text{T -Temperature}\end{array}$

Boyle’s law: Boyle’s law states that relationship between pressure of the gas and volume. That is pressure is inversely proportional to volume.

$\text{Pressure}\text{α}\frac{\text{1}}{\text{Volume}}$

Charles’s law: This law states that relationship between volume of an ideal gas and temperature at constant pressure. That is volume is directly proportional to temperature.

$\text{Volume α Temperature}$

c)

Interpretation Introduction

Interpretation: The qualitative graphs that distinguish between the following properties have to be drawn.

T versus V at constant P

Concept Introduction

Ideal gas law: This law expressed by following equation is,

$\text{PV = nRT}$

Where,

$\begin{array}{l}\text{P - Pressure}\\ \text{V - volume}\\ \text{n - Number of moles}\\ \text{R - Gasconstant}\\ \text{T -Temperature}\end{array}$

Boyle’s law: Boyle’s law states that relationship between pressure of the gas and volume. That is pressure is inversely proportional to volume.

$\text{Pressure}\text{α}\frac{\text{1}}{\text{Volume}}$

Charles’s law: This law states that relationship between volume of an ideal gas and temperature at constant pressure. That is volume is directly proportional to temperature.

$\text{Volume α Temperature}$

d)

Interpretation Introduction

Interpretation: The qualitative graphs that distinguish between the following properties have to be drawn.

P versus V at constant T

Concept Introduction

Ideal gas law: This law expressed by following equation is,

$\text{PV = nRT}$

Where,

$\begin{array}{l}\text{P - Pressure}\\ \text{V - volume}\\ \text{n - Number of moles}\\ \text{R - Gasconstant}\\ \text{T -Temperature}\end{array}$

Boyle’s law: Boyle’s law states that relationship between pressure of the gas and volume. That is pressure is inversely proportional to volume.

$\text{Pressure}\text{α}\frac{\text{1}}{\text{Volume}}$

Charles’s law: This law states that relationship between volume of an ideal gas and temperature at constant pressure. That is volume is directly proportional to temperature.

$\text{Volume α Temperature}$

e)

Interpretation Introduction

Interpretation: The qualitative graphs that distinguish between the following properties have to be drawn.

P versus $\frac{\text{1}}{\text{V}}$ at constant T

Concept Introduction

Ideal gas law: This law expressed by following equation is,

$\text{PV = nRT}$

Where,

$\begin{array}{l}\text{P - Pressure}\\ \text{V - volume}\\ \text{n - Number of moles}\\ \text{R - Gasconstant}\\ \text{T -Temperature}\end{array}$

Boyle’s law: Boyle’s law states that relationship between pressure of the gas and volume. That is pressure is inversely proportional to volume.

$\text{Pressure}\text{α}\frac{\text{1}}{\text{Volume}}$

Charles’s law: This law states that relationship between volume of an ideal gas and temperature at constant pressure. That is volume is directly proportional to temperature.

$\text{Volume α Temperature}$

f)

Interpretation Introduction

Interpretation: The qualitative graphs that distinguish between the following properties have to be drawn.

$\frac{\text{PV}}{\text{T}}$ versus P

Concept Introduction

Ideal gas law: This law expressed by following equation is,

$\text{PV = nRT}$

Where,

$\begin{array}{l}\text{P - Pressure}\\ \text{V - volume}\\ \text{n - Number of moles}\\ \text{R - Gasconstant}\\ \text{T -Temperature}\end{array}$

Boyle’s law: Boyle’s law states that relationship between pressure of the gas and volume. That is pressure is inversely proportional to volume.

$\text{Pressure}\text{α}\frac{\text{1}}{\text{Volume}}$

Charles’s law: This law states that relationship between volume of an ideal gas and temperature at constant pressure. That is volume is directly proportional to temperature.

$\text{Volume α Temperature}$