The SF 6 gas behaves more ideally at 150 ° C or at 20 ° C is to be explained. Concept introduction: Gases that obey the ideal gas equation at all temperature and pressure are known as ideal gas. The ideal gas equation can be expressed as follows, P V = n R T Here, P is the pressure, V is the volume, T is the temperature, n is the mole of the gas and R is the gas constant. The expression of van der Waals equation is as follows: ( P + n 2 a V 2 ) ( V − n b ) = n R T Here, P is the pressure, V is the volume, T is the temperature, n is the mole of the gas, R is the gas constant, a and b are van der Waals constants. The van der waals constants are depends upon the nature of gas, The value of a is greater than b . At low pressure and high temperature, real gas will obey the gas laws. The compressibility factor equation can be given as follows: Z = P V R T Here, P is the pressure, V is the volume, T is the temperature, Z is the compressibility factor, n is the mole of the gas and R is the gas constant. Z = 1 , that means gas shows ideal behaviour at all temperature and pressure. At high pressure, Z > 1 , the gas has less compressibility and more replusive force between the gas molecule. It shows positive deviation from ideal behaviour. At low pressure, Z < 1 , the gas has high compressibility and more attractive force between the gas molecules. It shows negative deviation from ideal behaviour.

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Answer 1

Question

Chapter 5, Problem 5.87P

Interpretation Introduction

Interpretation:

The $SF6$ gas behaves more ideally at $150 °C$ or at $20 °C$ is to be explained.

Concept introduction:

Gases that obey the ideal gas equation at all temperature and pressure are known as ideal gas.

The ideal gas equation can be expressed as follows,

$PV=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas and $R$ is the gas constant.

The expression of van der Waals equation is as follows:

$(P+n2aV2)(V−nb)=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas, $R$ is the gas constant, $a$ and $b$ are van der Waals constants.

The van der waals constants are depends upon the nature of gas, The value of $a$ is greater than $b$ .

At low pressure and high temperature, real gas will obey the gas laws.

The compressibility factor equation can be given as follows:

$Z=PVRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $Z$ is the compressibility factor, $n$ is the mole of the gas and $R$ is the gas constant.

$Z=1$ , that means gas shows ideal behaviour at all temperature and pressure.

At high pressure, $Z>1$ , the gas has less compressibility and more replusive force between the gas molecule. It shows positive deviation from ideal behaviour.

At low pressure, $Z<1$ , the gas has high compressibility and more attractive force between the gas molecules. It shows negative deviation from ideal behaviour.

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Answer 2

Question

Chapter 5, Problem 5.87P

Interpretation Introduction

Interpretation:

The $SF6$ gas behaves more ideally at $150 °C$ or at $20 °C$ is to be explained.

Concept introduction:

Gases that obey the ideal gas equation at all temperature and pressure are known as ideal gas.

The ideal gas equation can be expressed as follows,

$PV=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas and $R$ is the gas constant.

The expression of van der Waals equation is as follows:

$(P+n2aV2)(V−nb)=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas, $R$ is the gas constant, $a$ and $b$ are van der Waals constants.

The van der waals constants are depends upon the nature of gas, The value of $a$ is greater than $b$ .

At low pressure and high temperature, real gas will obey the gas laws.

The compressibility factor equation can be given as follows:

$Z=PVRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $Z$ is the compressibility factor, $n$ is the mole of the gas and $R$ is the gas constant.

$Z=1$ , that means gas shows ideal behaviour at all temperature and pressure.

At high pressure, $Z>1$ , the gas has less compressibility and more replusive force between the gas molecule. It shows positive deviation from ideal behaviour.

At low pressure, $Z<1$ , the gas has high compressibility and more attractive force between the gas molecules. It shows negative deviation from ideal behaviour.

Expert Solution & Answer

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Answer 3

Question

Chapter 5, Problem 5.87P

Interpretation Introduction

Interpretation:

The $SF6$ gas behaves more ideally at $150 °C$ or at $20 °C$ is to be explained.

Concept introduction:

Gases that obey the ideal gas equation at all temperature and pressure are known as ideal gas.

The ideal gas equation can be expressed as follows,

$PV=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas and $R$ is the gas constant.

The expression of van der Waals equation is as follows:

$(P+n2aV2)(V−nb)=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas, $R$ is the gas constant, $a$ and $b$ are van der Waals constants.

The van der waals constants are depends upon the nature of gas, The value of $a$ is greater than $b$ .

At low pressure and high temperature, real gas will obey the gas laws.

The compressibility factor equation can be given as follows:

$Z=PVRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $Z$ is the compressibility factor, $n$ is the mole of the gas and $R$ is the gas constant.

$Z=1$ , that means gas shows ideal behaviour at all temperature and pressure.

At high pressure, $Z>1$ , the gas has less compressibility and more replusive force between the gas molecule. It shows positive deviation from ideal behaviour.

At low pressure, $Z<1$ , the gas has high compressibility and more attractive force between the gas molecules. It shows negative deviation from ideal behaviour.

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Answer 4

Question

Chapter 5, Problem 5.87P

Interpretation Introduction

Interpretation:

The $SF6$ gas behaves more ideally at $150 °C$ or at $20 °C$ is to be explained.

Concept introduction:

Gases that obey the ideal gas equation at all temperature and pressure are known as ideal gas.

The ideal gas equation can be expressed as follows,

$PV=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas and $R$ is the gas constant.

The expression of van der Waals equation is as follows:

$(P+n2aV2)(V−nb)=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas, $R$ is the gas constant, $a$ and $b$ are van der Waals constants.

The van der waals constants are depends upon the nature of gas, The value of $a$ is greater than $b$ .

At low pressure and high temperature, real gas will obey the gas laws.

The compressibility factor equation can be given as follows:

$Z=PVRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $Z$ is the compressibility factor, $n$ is the mole of the gas and $R$ is the gas constant.

$Z=1$ , that means gas shows ideal behaviour at all temperature and pressure.

At high pressure, $Z>1$ , the gas has less compressibility and more replusive force between the gas molecule. It shows positive deviation from ideal behaviour.

At low pressure, $Z<1$ , the gas has high compressibility and more attractive force between the gas molecules. It shows negative deviation from ideal behaviour.

Expert Solution & Answer

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Answer 5

Chapter 5, Problem 5.87P

Interpretation Introduction

Interpretation:

The $SF6$ gas behaves more ideally at $150 °C$ or at $20 °C$ is to be explained.

Concept introduction:

Gases that obey the ideal gas equation at all temperature and pressure are known as ideal gas.

The ideal gas equation can be expressed as follows,

$PV=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas and $R$ is the gas constant.

The expression of van der Waals equation is as follows:

$(P+n2aV2)(V−nb)=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas, $R$ is the gas constant, $a$ and $b$ are van der Waals constants.

The van der waals constants are depends upon the nature of gas, The value of $a$ is greater than $b$ .

At low pressure and high temperature, real gas will obey the gas laws.

The compressibility factor equation can be given as follows:

$Z=PVRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $Z$ is the compressibility factor, $n$ is the mole of the gas and $R$ is the gas constant.

$Z=1$ , that means gas shows ideal behaviour at all temperature and pressure.

At high pressure, $Z>1$ , the gas has less compressibility and more replusive force between the gas molecule. It shows positive deviation from ideal behaviour.

At low pressure, $Z<1$ , the gas has high compressibility and more attractive force between the gas molecules. It shows negative deviation from ideal behaviour.

Answer 6

Chapter 5, Problem 5.87P

Interpretation Introduction

Interpretation:

The $SF6$ gas behaves more ideally at $150 °C$ or at $20 °C$ is to be explained.

Concept introduction:

Gases that obey the ideal gas equation at all temperature and pressure are known as ideal gas.

The ideal gas equation can be expressed as follows,

$PV=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas and $R$ is the gas constant.

The expression of van der Waals equation is as follows:

$(P+n2aV2)(V−nb)=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas, $R$ is the gas constant, $a$ and $b$ are van der Waals constants.

The van der waals constants are depends upon the nature of gas, The value of $a$ is greater than $b$ .

At low pressure and high temperature, real gas will obey the gas laws.

The compressibility factor equation can be given as follows:

$Z=PVRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $Z$ is the compressibility factor, $n$ is the mole of the gas and $R$ is the gas constant.

$Z=1$ , that means gas shows ideal behaviour at all temperature and pressure.

At high pressure, $Z>1$ , the gas has less compressibility and more replusive force between the gas molecule. It shows positive deviation from ideal behaviour.

At low pressure, $Z<1$ , the gas has high compressibility and more attractive force between the gas molecules. It shows negative deviation from ideal behaviour.

Answer 7

Chapter 5, Problem 5.87P

Interpretation Introduction

Interpretation:

The $SF6$ gas behaves more ideally at $150 °C$ or at $20 °C$ is to be explained.

Concept introduction:

Gases that obey the ideal gas equation at all temperature and pressure are known as ideal gas.

The ideal gas equation can be expressed as follows,

$PV=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas and $R$ is the gas constant.

The expression of van der Waals equation is as follows:

$(P+n2aV2)(V−nb)=nRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $n$ is the mole of the gas, $R$ is the gas constant, $a$ and $b$ are van der Waals constants.

The van der waals constants are depends upon the nature of gas, The value of $a$ is greater than $b$ .

At low pressure and high temperature, real gas will obey the gas laws.

The compressibility factor equation can be given as follows:

$Z=PVRT$

Here, $P$ is the pressure, $V$ is the volume, $T$ is the temperature, $Z$ is the compressibility factor, $n$ is the mole of the gas and $R$ is the gas constant.

$Z=1$ , that means gas shows ideal behaviour at all temperature and pressure.

At high pressure, $Z>1$ , the gas has less compressibility and more replusive force between the gas molecule. It shows positive deviation from ideal behaviour.

At low pressure, $Z<1$ , the gas has high compressibility and more attractive force between the gas molecules. It shows negative deviation from ideal behaviour.

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 5.2 - The CO2 released from another limestone sample is...Ch. 5.2 - Prob. 5.1BFP Ch. 5.3 - Prob. 5.2AFP Ch. 5.3 - Prob. 5.2BFP Ch. 5.3 - Prob. 5.3AFP Ch. 5.3 - Prob. 5.3BFP Ch. 5.3 - Prob. 5.4AFP Ch. 5.3 - A balloon filled with 1.26 g of nitrogen gas has a...Ch. 5.3 - Prob. 5.5AFP Ch. 5.3 - Prob. 5.5BFP

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