Amount of heat whether absorbed or released is to be calculated when given amount work is done by the system on surrounding. Concept introduction: The first law of thermodynamics states that heat is a form of energy. Energy can neither be created nor be destroyed in an isolated system. Equation for the first law is as follows: Δ U = q + w Here, U is the internal energy of the system, q is the heat given to or removed from the system, and w is the work done by or to the system. If the sign of q is positive, heat is absorbed by the system. If the sign of q is negative, heat is released by the system.

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Answer 1

Question

Chapter 5, Problem 16QP

Interpretation Introduction

Interpretation:

Amount of heat whether absorbed or released is to be calculated when given amount work is done by the system on surrounding.

Concept introduction:

The first law of thermodynamics states that heat is a form of energy. Energy can neither be created nor be destroyed in an isolated system.

Equation for the first law is as follows:

ΔU=q+w

Here, U is the internal energy of the system, q is the heat given to or removed from the system, and w is the work done by or to the system.

If the sign of q is positive, heat is absorbed by the system.

If the sign of q is negative, heat is released by the system.

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Answer 2

Question

Chapter 5, Problem 16QP

Interpretation Introduction

Interpretation:

Amount of heat whether absorbed or released is to be calculated when given amount work is done by the system on surrounding.

Concept introduction:

The first law of thermodynamics states that heat is a form of energy. Energy can neither be created nor be destroyed in an isolated system.

Equation for the first law is as follows:

ΔU=q+w

Here, U is the internal energy of the system, q is the heat given to or removed from the system, and w is the work done by or to the system.

If the sign of q is positive, heat is absorbed by the system.

If the sign of q is negative, heat is released by the system.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 5, Problem 16QP

Interpretation Introduction

Interpretation:

Amount of heat whether absorbed or released is to be calculated when given amount work is done by the system on surrounding.

Concept introduction:

The first law of thermodynamics states that heat is a form of energy. Energy can neither be created nor be destroyed in an isolated system.

Equation for the first law is as follows:

ΔU=q+w

Here, U is the internal energy of the system, q is the heat given to or removed from the system, and w is the work done by or to the system.

If the sign of q is positive, heat is absorbed by the system.

If the sign of q is negative, heat is released by the system.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 5, Problem 16QP

Interpretation Introduction

Interpretation:

Amount of heat whether absorbed or released is to be calculated when given amount work is done by the system on surrounding.

Concept introduction:

The first law of thermodynamics states that heat is a form of energy. Energy can neither be created nor be destroyed in an isolated system.

Equation for the first law is as follows:

ΔU=q+w

Here, U is the internal energy of the system, q is the heat given to or removed from the system, and w is the work done by or to the system.

If the sign of q is positive, heat is absorbed by the system.

If the sign of q is negative, heat is released by the system.

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 5

Chapter 5, Problem 16QP

Interpretation Introduction

Interpretation:

Amount of heat whether absorbed or released is to be calculated when given amount work is done by the system on surrounding.

Concept introduction:

The first law of thermodynamics states that heat is a form of energy. Energy can neither be created nor be destroyed in an isolated system.

Equation for the first law is as follows:

ΔU=q+w

Here, U is the internal energy of the system, q is the heat given to or removed from the system, and w is the work done by or to the system.

If the sign of q is positive, heat is absorbed by the system.

If the sign of q is negative, heat is released by the system.

Answer 6

Chapter 5, Problem 16QP

Interpretation Introduction

Interpretation:

Amount of heat whether absorbed or released is to be calculated when given amount work is done by the system on surrounding.

Concept introduction:

The first law of thermodynamics states that heat is a form of energy. Energy can neither be created nor be destroyed in an isolated system.

Equation for the first law is as follows:

ΔU=q+w

Here, U is the internal energy of the system, q is the heat given to or removed from the system, and w is the work done by or to the system.

If the sign of q is positive, heat is absorbed by the system.

If the sign of q is negative, heat is released by the system.

Answer 7

Chapter 5, Problem 16QP

Interpretation Introduction

Interpretation:

Amount of heat whether absorbed or released is to be calculated when given amount work is done by the system on surrounding.

Concept introduction:

The first law of thermodynamics states that heat is a form of energy. Energy can neither be created nor be destroyed in an isolated system.

Equation for the first law is as follows:

ΔU=q+w

Here, U is the internal energy of the system, q is the heat given to or removed from the system, and w is the work done by or to the system.

If the sign of q is positive, heat is absorbed by the system.

If the sign of q is negative, heat is released by the system.

Answer 8

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Answer 9

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Answer 10

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Answer 11

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Solution Summary: The author explains that the first law of thermodynamics states that heat is a form of energy. It can neither be created nor destroyed in an isolated system.

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