The volume of balloon “if the amount of hydrogen remains the same” should be calculated. Concept introduction: Here, we are using the concept of different gaseous law which are combined to form a combined gaseous law. ► Boyle’s Law: It states that at constant temperature, the pressure of the gas has inverse relation with volume P α 1 V ► Charles’ Law: It states that at constant pressure, the volume is directly proportional to the temperature V α T ► Gay-Lussac’s law: It states that at constant volume, the pressure of the gas has direct relation with temperature P α T ► Now by combining the three law we get a relationship between pressure, volume and temperature which is known as combined gas equation P 1 V 1 T 1 = P 2 V 2 T 2 Given: Initial volume of the balloon, V 1 = 31000 L Pressure, P 1 = 755 mmHg Temperature of the gas, T 1 = 22 0 C At 1000 m altitude Pressure of the gas, P 2 = 658 mmHg Temperature of the gas, T 2 = − 8 0 C

Question

Want to see the full answer?

Answer 1

Question

Chapter 8, Problem 8.81AQAP

Interpretation Introduction

Interpretation:

The volume of balloon “if the amount of hydrogen remains the same” should be calculated.

Concept introduction:

Here, we are using the concept of different gaseous law which are combined to form a combined gaseous law.

► Boyle’s Law: It states that at constant temperature, the pressure of the gas has inverse relation with volume

$P α \frac{1}{V}$

► Charles’ Law: It states that at constant pressure, the volume is directly proportional to the temperature

$V α T$

► Gay-Lussac’s law: It states that at constant volume, the pressure of the gas has direct relation with temperature

$P α T$

► Now by combining the three law we get a relationship between pressure, volume and temperature which is known as combined gas equation

$\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$

Given:

Initial volume of the balloon, $V_{1} = 31000 L$

Pressure, $P_{1} = 755 mmHg$

Temperature of the gas, $T_{1} = 22^{0} C$

At $1000 m$ altitude

Pressure of the gas, $P_{2} = 658 mmHg$

Temperature of the gas, $T_{2} = - 8^{0} C$

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

One step of glycolysis is a retro-aldol reaction (aldolase) to produce ATP.Below is the aldol reaction of the equilibrium. Show the mechanism for the base catalyzed reaction. *see image

Provide the missing information. *see image

Why does the following reaction lead to poor yields? Correct the reaction. *see image

Answer 2

Question

Chapter 8, Problem 8.81AQAP

Interpretation Introduction

Interpretation:

The volume of balloon “if the amount of hydrogen remains the same” should be calculated.

Concept introduction:

Here, we are using the concept of different gaseous law which are combined to form a combined gaseous law.

► Boyle’s Law: It states that at constant temperature, the pressure of the gas has inverse relation with volume

$P α \frac{1}{V}$

► Charles’ Law: It states that at constant pressure, the volume is directly proportional to the temperature

$V α T$

► Gay-Lussac’s law: It states that at constant volume, the pressure of the gas has direct relation with temperature

$P α T$

► Now by combining the three law we get a relationship between pressure, volume and temperature which is known as combined gas equation

$\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$

Given:

Initial volume of the balloon, $V_{1} = 31000 L$

Pressure, $P_{1} = 755 mmHg$

Temperature of the gas, $T_{1} = 22^{0} C$

At $1000 m$ altitude

Pressure of the gas, $P_{2} = 658 mmHg$

Temperature of the gas, $T_{2} = - 8^{0} C$

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 8, Problem 8.81AQAP

Interpretation Introduction

Interpretation:

The volume of balloon “if the amount of hydrogen remains the same” should be calculated.

Concept introduction:

Here, we are using the concept of different gaseous law which are combined to form a combined gaseous law.

► Boyle’s Law: It states that at constant temperature, the pressure of the gas has inverse relation with volume

$P α \frac{1}{V}$

► Charles’ Law: It states that at constant pressure, the volume is directly proportional to the temperature

$V α T$

► Gay-Lussac’s law: It states that at constant volume, the pressure of the gas has direct relation with temperature

$P α T$

► Now by combining the three law we get a relationship between pressure, volume and temperature which is known as combined gas equation

$\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$

Given:

Initial volume of the balloon, $V_{1} = 31000 L$

Pressure, $P_{1} = 755 mmHg$

Temperature of the gas, $T_{1} = 22^{0} C$

At $1000 m$ altitude

Pressure of the gas, $P_{2} = 658 mmHg$

Temperature of the gas, $T_{2} = - 8^{0} C$

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 8, Problem 8.81AQAP

Interpretation Introduction

Interpretation:

The volume of balloon “if the amount of hydrogen remains the same” should be calculated.

Concept introduction:

Here, we are using the concept of different gaseous law which are combined to form a combined gaseous law.

► Boyle’s Law: It states that at constant temperature, the pressure of the gas has inverse relation with volume

$P α \frac{1}{V}$

► Charles’ Law: It states that at constant pressure, the volume is directly proportional to the temperature

$V α T$

► Gay-Lussac’s law: It states that at constant volume, the pressure of the gas has direct relation with temperature

$P α T$

► Now by combining the three law we get a relationship between pressure, volume and temperature which is known as combined gas equation

$\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$

Given:

Initial volume of the balloon, $V_{1} = 31000 L$

Pressure, $P_{1} = 755 mmHg$

Temperature of the gas, $T_{1} = 22^{0} C$

At $1000 m$ altitude

Pressure of the gas, $P_{2} = 658 mmHg$

Temperature of the gas, $T_{2} = - 8^{0} C$

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 8, Problem 8.81AQAP

Interpretation Introduction

Interpretation:

The volume of balloon “if the amount of hydrogen remains the same” should be calculated.

Concept introduction:

Here, we are using the concept of different gaseous law which are combined to form a combined gaseous law.

► Boyle’s Law: It states that at constant temperature, the pressure of the gas has inverse relation with volume

$P α \frac{1}{V}$

► Charles’ Law: It states that at constant pressure, the volume is directly proportional to the temperature

$V α T$

► Gay-Lussac’s law: It states that at constant volume, the pressure of the gas has direct relation with temperature

$P α T$

► Now by combining the three law we get a relationship between pressure, volume and temperature which is known as combined gas equation

$\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$

Given:

Initial volume of the balloon, $V_{1} = 31000 L$

Pressure, $P_{1} = 755 mmHg$

Temperature of the gas, $T_{1} = 22^{0} C$

At $1000 m$ altitude

Pressure of the gas, $P_{2} = 658 mmHg$

Temperature of the gas, $T_{2} = - 8^{0} C$

Answer 6

Chapter 8, Problem 8.81AQAP

Interpretation Introduction

Interpretation:

The volume of balloon “if the amount of hydrogen remains the same” should be calculated.

Concept introduction:

Here, we are using the concept of different gaseous law which are combined to form a combined gaseous law.

► Boyle’s Law: It states that at constant temperature, the pressure of the gas has inverse relation with volume

$P α \frac{1}{V}$

► Charles’ Law: It states that at constant pressure, the volume is directly proportional to the temperature

$V α T$

► Gay-Lussac’s law: It states that at constant volume, the pressure of the gas has direct relation with temperature

$P α T$

► Now by combining the three law we get a relationship between pressure, volume and temperature which is known as combined gas equation

$\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$

Given:

Initial volume of the balloon, $V_{1} = 31000 L$

Pressure, $P_{1} = 755 mmHg$

Temperature of the gas, $T_{1} = 22^{0} C$

At $1000 m$ altitude

Pressure of the gas, $P_{2} = 658 mmHg$

Temperature of the gas, $T_{2} = - 8^{0} C$

Answer 7

Chapter 8, Problem 8.81AQAP

Interpretation Introduction

Interpretation:

The volume of balloon “if the amount of hydrogen remains the same” should be calculated.

Concept introduction:

Here, we are using the concept of different gaseous law which are combined to form a combined gaseous law.

► Boyle’s Law: It states that at constant temperature, the pressure of the gas has inverse relation with volume

$P α \frac{1}{V}$

► Charles’ Law: It states that at constant pressure, the volume is directly proportional to the temperature

$V α T$

► Gay-Lussac’s law: It states that at constant volume, the pressure of the gas has direct relation with temperature

$P α T$

► Now by combining the three law we get a relationship between pressure, volume and temperature which is known as combined gas equation

$\frac{P_{1} V_{1}}{T_{1}} = \frac{P_{2} V_{2}}{T_{2}}$

Given:

Initial volume of the balloon, $V_{1} = 31000 L$

Pressure, $P_{1} = 755 mmHg$

Temperature of the gas, $T_{1} = 22^{0} C$

At $1000 m$ altitude

Pressure of the gas, $P_{2} = 658 mmHg$

Temperature of the gas, $T_{2} = - 8^{0} C$

Answer 8

Expert Solution & Answer

Answer 9

Expert Solution & Answer

Answer 10

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 11

Ch. 8.1 - Prob. 8.1QAP Ch. 8.1 - Prob. 8.2QAP Ch. 8.1 - Prob. 8.3QAP Ch. 8.1 - Prob. 8.4QAP Ch. 8.1 - Prob. 8.5QAP Ch. 8.1 - Prob. 8.6QAP Ch. 8.1 - Prob. 8.7QAP Ch. 8.1 - Prob. 8.8QAP Ch. 8.2 - Why do scuba divers need to exhale air when they...Ch. 8.2 - Why does a sealed bag of chips expand when you...

Concept explainers

Videos

Want to see the full answer?

Chapter 8 Solutions