The change in temperature for 1 mole of an ideal gas needs to be determined if heat released is 425 J and work done on the system is 185 J. Concept Introduction: The change in internal energy is calculated as follows: Δ U = n C V . m ( T f − T i ) Here, n is number of moles, C V , m is molar heat at constant volume and T is temperature. The work done is represented as follows: w = − P external Δ V Here, P is external pressure and Δ V is change in volume. The enthalpy of a reaction is represented as follows: Δ H = Δ U + n R Δ T Here, n is number of moles, R is Universal gas constant and Δ T is change in temperature.

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Answer 1

Question

Chapter 2, Problem 2.34NP

(a)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat released is 425 J and work done on the system is 185 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

(b)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat absorbed is 315 J and work done by the system is 315 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

(c)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if no heat is involved and work done on the system is 225 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

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Answer 2

Question

Chapter 2, Problem 2.34NP

(a)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat released is 425 J and work done on the system is 185 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

(b)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat absorbed is 315 J and work done by the system is 315 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

(c)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if no heat is involved and work done on the system is 225 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 2, Problem 2.34NP

(a)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat released is 425 J and work done on the system is 185 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

(b)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat absorbed is 315 J and work done by the system is 315 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

(c)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if no heat is involved and work done on the system is 225 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 2, Problem 2.34NP

(a)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat released is 425 J and work done on the system is 185 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

(b)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat absorbed is 315 J and work done by the system is 315 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

(c)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if no heat is involved and work done on the system is 225 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 2, Problem 2.34NP

(a)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat released is 425 J and work done on the system is 185 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

(b)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat absorbed is 315 J and work done by the system is 315 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

(c)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if no heat is involved and work done on the system is 225 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

Answer 6

Chapter 2, Problem 2.34NP

(a)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat released is 425 J and work done on the system is 185 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

Answer 7

Chapter 2, Problem 2.34NP

(a)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat released is 425 J and work done on the system is 185 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

Answer 8

(b)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat absorbed is 315 J and work done by the system is 315 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

Answer 9

(b)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if heat absorbed is 315 J and work done by the system is 315 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

Answer 10

(c)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if no heat is involved and work done on the system is 225 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

Answer 11

(c)

Interpretation Introduction

Interpretation: The change in temperature for 1 mole of an ideal gas needs to be determined if no heat is involved and work done on the system is 225 J.

Concept Introduction: The change in internal energy is calculated as follows:

ΔU=nCV.m(Tf−Ti)

Here, n is number of moles, CV,m is molar heat at constant volume and T is temperature.

The work done is represented as follows:

w=−PexternalΔV

Here, P is external pressure and ΔV is change in volume.

The enthalpy of a reaction is represented as follows:

ΔH=ΔU+nRΔT

Here, n is number of moles, R is Universal gas constant and ΔT is change in temperature.

Answer 12

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

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Answer 15

Ch. 2 - Prob. 2.1CP Ch. 2 - Prob. 2.2CP Ch. 2 - Prob. 2.3CP Ch. 2 - Prob. 2.4CP Ch. 2 - Prob. 2.5CP Ch. 2 - Prob. 2.6CP Ch. 2 - Prob. 2.7CP Ch. 2 - Prob. 2.8CP Ch. 2 - Prob. 2.9CP Ch. 2 - Prob. 2.10CP

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