Whether the butane kept at 25 ° C and 1 atm or the nitrogen kept at 25 ° C and 1 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained. Concept Introduction: In general, it has been found that gases obey the ideal gas law at fairly low pressure and high-temperature conditions and deviate from ideality at high pressure or very low temperatures. For most of the gases, ideal gas law is followed for temperatures far much above or below the condensation point. The condensation point or the boiling point of a gas is a particular temperature when the gas molecules condense as a result of forces of attraction and form a liquid. Since liquids do not follow ideal gas law the conditions near the condensation point as that of exceedingly low temperatures are not suitable for any gas to follow the ideal gas law.

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Answer 1

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Definition Definition Law that is the combined form of Boyle's Law, Charles's Law, and Avogadro's Law. This law is obeyed by all ideal gas. Boyle's Law states that pressure is inversely proportional to volume. Charles's Law states that volume is in direct relation to temperature. Avogadro's Law shows that volume is in direct relation to the number of moles in the gas. The mathematical equation for the ideal gas law equation has been formulated by taking all the equations into account: PV=nRT Where P = pressure of the ideal gas V = volume of the ideal gas n = amount of ideal gas measured in moles R = universal gas constant and its value is 8.314 J.K-1mol-1 T = temperature

Chapter 6, Problem 6.114QE

(a)

Interpretation Introduction

Interpretation:

Whether the butane kept at 25 °C and 1 atm or the nitrogen kept at 25 °C and 1 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

In general, it has been found that gases obey the ideal gas law at fairly low pressure and high-temperature conditions and deviate from ideality at high pressure or very low temperatures.

For most of the gases, ideal gas law is followed for temperatures far much above or below the condensation point. The condensation point or the boiling point of a gas is a particular temperature when the gas molecules condense as a result of forces of attraction and form a liquid. Since liquids do not follow ideal gas law the conditions near the condensation point as that of exceedingly low temperatures are not suitable for any gas to follow the ideal gas law.

(b)

Interpretation Introduction

Interpretation:

Whether O2 gas kept at 0.50 atm or O2 kept at 150 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

Whether argon kept at −160 °C and 1 atm or sulfur dioxide kept at 10 °C obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

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Answer 2

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Definition Definition Law that is the combined form of Boyle's Law, Charles's Law, and Avogadro's Law. This law is obeyed by all ideal gas. Boyle's Law states that pressure is inversely proportional to volume. Charles's Law states that volume is in direct relation to temperature. Avogadro's Law shows that volume is in direct relation to the number of moles in the gas. The mathematical equation for the ideal gas law equation has been formulated by taking all the equations into account: PV=nRT Where P = pressure of the ideal gas V = volume of the ideal gas n = amount of ideal gas measured in moles R = universal gas constant and its value is 8.314 J.K-1mol-1 T = temperature

Chapter 6, Problem 6.114QE

(a)

Interpretation Introduction

Interpretation:

Whether the butane kept at 25 °C and 1 atm or the nitrogen kept at 25 °C and 1 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

In general, it has been found that gases obey the ideal gas law at fairly low pressure and high-temperature conditions and deviate from ideality at high pressure or very low temperatures.

For most of the gases, ideal gas law is followed for temperatures far much above or below the condensation point. The condensation point or the boiling point of a gas is a particular temperature when the gas molecules condense as a result of forces of attraction and form a liquid. Since liquids do not follow ideal gas law the conditions near the condensation point as that of exceedingly low temperatures are not suitable for any gas to follow the ideal gas law.

(b)

Interpretation Introduction

Interpretation:

Whether O2 gas kept at 0.50 atm or O2 kept at 150 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

Whether argon kept at −160 °C and 1 atm or sulfur dioxide kept at 10 °C obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

Expert Solution & Answer

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See solution

Answer 3

Question

Definition Definition Law that is the combined form of Boyle's Law, Charles's Law, and Avogadro's Law. This law is obeyed by all ideal gas. Boyle's Law states that pressure is inversely proportional to volume. Charles's Law states that volume is in direct relation to temperature. Avogadro's Law shows that volume is in direct relation to the number of moles in the gas. The mathematical equation for the ideal gas law equation has been formulated by taking all the equations into account: PV=nRT Where P = pressure of the ideal gas V = volume of the ideal gas n = amount of ideal gas measured in moles R = universal gas constant and its value is 8.314 J.K-1mol-1 T = temperature

Chapter 6, Problem 6.114QE

(a)

Interpretation Introduction

Interpretation:

Whether the butane kept at 25 °C and 1 atm or the nitrogen kept at 25 °C and 1 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

In general, it has been found that gases obey the ideal gas law at fairly low pressure and high-temperature conditions and deviate from ideality at high pressure or very low temperatures.

For most of the gases, ideal gas law is followed for temperatures far much above or below the condensation point. The condensation point or the boiling point of a gas is a particular temperature when the gas molecules condense as a result of forces of attraction and form a liquid. Since liquids do not follow ideal gas law the conditions near the condensation point as that of exceedingly low temperatures are not suitable for any gas to follow the ideal gas law.

(b)

Interpretation Introduction

Interpretation:

Whether O2 gas kept at 0.50 atm or O2 kept at 150 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

Whether argon kept at −160 °C and 1 atm or sulfur dioxide kept at 10 °C obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

Expert Solution & Answer

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Answer 4

Question

Definition Definition Law that is the combined form of Boyle's Law, Charles's Law, and Avogadro's Law. This law is obeyed by all ideal gas. Boyle's Law states that pressure is inversely proportional to volume. Charles's Law states that volume is in direct relation to temperature. Avogadro's Law shows that volume is in direct relation to the number of moles in the gas. The mathematical equation for the ideal gas law equation has been formulated by taking all the equations into account: PV=nRT Where P = pressure of the ideal gas V = volume of the ideal gas n = amount of ideal gas measured in moles R = universal gas constant and its value is 8.314 J.K-1mol-1 T = temperature

Chapter 6, Problem 6.114QE

(a)

Interpretation Introduction

Interpretation:

Whether the butane kept at 25 °C and 1 atm or the nitrogen kept at 25 °C and 1 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

In general, it has been found that gases obey the ideal gas law at fairly low pressure and high-temperature conditions and deviate from ideality at high pressure or very low temperatures.

For most of the gases, ideal gas law is followed for temperatures far much above or below the condensation point. The condensation point or the boiling point of a gas is a particular temperature when the gas molecules condense as a result of forces of attraction and form a liquid. Since liquids do not follow ideal gas law the conditions near the condensation point as that of exceedingly low temperatures are not suitable for any gas to follow the ideal gas law.

(b)

Interpretation Introduction

Interpretation:

Whether O2 gas kept at 0.50 atm or O2 kept at 150 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

Whether argon kept at −160 °C and 1 atm or sulfur dioxide kept at 10 °C obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

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Answer 5

Chapter 6, Problem 6.114QE

(a)

Interpretation Introduction

Interpretation:

Whether the butane kept at 25 °C and 1 atm or the nitrogen kept at 25 °C and 1 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

In general, it has been found that gases obey the ideal gas law at fairly low pressure and high-temperature conditions and deviate from ideality at high pressure or very low temperatures.

For most of the gases, ideal gas law is followed for temperatures far much above or below the condensation point. The condensation point or the boiling point of a gas is a particular temperature when the gas molecules condense as a result of forces of attraction and form a liquid. Since liquids do not follow ideal gas law the conditions near the condensation point as that of exceedingly low temperatures are not suitable for any gas to follow the ideal gas law.

(b)

Interpretation Introduction

Interpretation:

Whether O2 gas kept at 0.50 atm or O2 kept at 150 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

(c)

Interpretation Introduction

Interpretation:

Whether argon kept at −160 °C and 1 atm or sulfur dioxide kept at 10 °C obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

Answer 6

Chapter 6, Problem 6.114QE

(a)

Interpretation Introduction

Interpretation:

Whether the butane kept at 25 °C and 1 atm or the nitrogen kept at 25 °C and 1 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

In general, it has been found that gases obey the ideal gas law at fairly low pressure and high-temperature conditions and deviate from ideality at high pressure or very low temperatures.

For most of the gases, ideal gas law is followed for temperatures far much above or below the condensation point. The condensation point or the boiling point of a gas is a particular temperature when the gas molecules condense as a result of forces of attraction and form a liquid. Since liquids do not follow ideal gas law the conditions near the condensation point as that of exceedingly low temperatures are not suitable for any gas to follow the ideal gas law.

Answer 7

Chapter 6, Problem 6.114QE

(a)

Interpretation Introduction

Interpretation:

Whether the butane kept at 25 °C and 1 atm or the nitrogen kept at 25 °C and 1 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

In general, it has been found that gases obey the ideal gas law at fairly low pressure and high-temperature conditions and deviate from ideality at high pressure or very low temperatures.

For most of the gases, ideal gas law is followed for temperatures far much above or below the condensation point. The condensation point or the boiling point of a gas is a particular temperature when the gas molecules condense as a result of forces of attraction and form a liquid. Since liquids do not follow ideal gas law the conditions near the condensation point as that of exceedingly low temperatures are not suitable for any gas to follow the ideal gas law.

Answer 8

(b)

Interpretation Introduction

Interpretation:

Whether O2 gas kept at 0.50 atm or O2 kept at 150 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

Answer 9

(b)

Interpretation Introduction

Interpretation:

Whether O2 gas kept at 0.50 atm or O2 kept at 150 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

Answer 10

(c)

Interpretation Introduction

Interpretation:

Whether argon kept at −160 °C and 1 atm or sulfur dioxide kept at 10 °C obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

Answer 11

(c)

Interpretation Introduction

Interpretation:

Whether argon kept at −160 °C and 1 atm or sulfur dioxide kept at 10 °C obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

Answer 12

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Answer 13

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Answer 14

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Answer 15

Ch. 6 - Prob. 6.1QE Ch. 6 - Prob. 6.2QE Ch. 6 - Prob. 6.3QE Ch. 6 - Prob. 6.4QE Ch. 6 - Prob. 6.5QE Ch. 6 - Prob. 6.6QE Ch. 6 - Prob. 6.7QE Ch. 6 - Prob. 6.8QE Ch. 6 - Prob. 6.9QE Ch. 6 - Prob. 6.10QE

Solution Summary: The author explains that gases obey the ideal gas law at relatively low pressure and high-temperature conditions and deviate from ideality at high pressure or very low temperatures.

Concept explainers

Interpretation:

Whether O2 gas kept at 0.50 atm or O2 kept at 150 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

Interpretation:

Whether argon kept at −160 °C and 1 atm or sulfur dioxide kept at 10 °C obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

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Chapter 6 Solutions

Solution Summary: The author explains that gases obey the ideal gas law at relatively low pressure and high-temperature conditions and deviate from ideality at high pressure or very low temperatures.

Concept explainers

Interpretation: Whether O2 gas kept at 0.50 atm or O2 kept at 150 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained. Concept Introduction: Refer to part (a).

Interpretation: Whether argon kept at −160 °C and 1 atm or sulfur dioxide kept at 10 °C obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained. Concept Introduction: Refer to part (a).

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Chapter 6 Solutions

Interpretation:

Whether O2 gas kept at 0.50 atm or O2 kept at 150 atm obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).

Interpretation:

Whether argon kept at −160 °C and 1 atm or sulfur dioxide kept at 10 °C obeys the ideal gas law or not has to be predicted and the reason behind the choice has to be explained.

Concept Introduction:

Refer to part (a).