The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes a reversible adiabatic expansion and final pressure is 1/3 r d of the initial. Concept Introduction: The change in enthalpy for a process can be calculated as follows: Δ H = C P , m n Δ T Here, C P , m is molar heat capacity at constant pressure. Also, the change in internal energy as follows: Δ U = C V , m n Δ T Here, C V , m is molar heat capacity at constant volume. Also, Δ U = q + w Here, q is heat and w is work done. The ideal gas equation is represented as follows: P V = n R T Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

Question

Want to see the full answer?

Answer 1

Question

Chapter 5, Problem 5.16NP

(a)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes a reversible adiabatic expansion and final pressure is 1/3^r^d of the initial.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

(b)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an adiabatic expansion at constant external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

(c)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an expansion at zero external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

How many chiral centers/stereocenters are there in the following molecule? 1 2 3 4

Which of these correspond to the molecule: 2,5-dimethylheptane

Given the following data, determine the order of the reaction with respect to H2. H2(g) + 21Cl(g) → I2(g) + 2HCl(g) Experiment [H2] (torr) [ICI] (torr) Rate (M/s) 1 250 325 0.266 2 250 81 0.0665 3 50 325 0.266

Answer 2

Question

Chapter 5, Problem 5.16NP

(a)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes a reversible adiabatic expansion and final pressure is 1/3^r^d of the initial.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

(b)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an adiabatic expansion at constant external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

(c)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an expansion at zero external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

Chapter 5, Problem 5.16NP

(a)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes a reversible adiabatic expansion and final pressure is 1/3^r^d of the initial.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

(b)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an adiabatic expansion at constant external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

(c)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an expansion at zero external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

Chapter 5, Problem 5.16NP

(a)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes a reversible adiabatic expansion and final pressure is 1/3^r^d of the initial.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

(b)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an adiabatic expansion at constant external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

(c)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an expansion at zero external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

Chapter 5, Problem 5.16NP

(a)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes a reversible adiabatic expansion and final pressure is 1/3^r^d of the initial.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

(b)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an adiabatic expansion at constant external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

(c)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an expansion at zero external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

Answer 6

Chapter 5, Problem 5.16NP

(a)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes a reversible adiabatic expansion and final pressure is 1/3^r^d of the initial.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

Answer 7

Chapter 5, Problem 5.16NP

(a)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes a reversible adiabatic expansion and final pressure is 1/3^r^d of the initial.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

Answer 8

(b)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an adiabatic expansion at constant external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

Answer 9

(b)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an adiabatic expansion at constant external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

Answer 10

(c)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an expansion at zero external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

Answer 11

(c)

Interpretation Introduction

Interpretation: The value of heat, work done, change in internal energy, change in entropy and change in enthalpy needs to be determined if a gas undergoes an expansion at zero external pressure and final pressure is 1/3^r^d of the initial volume.

Concept Introduction:

The change in enthalpy for a process can be calculated as follows:

ΔH=CP,mnΔT

Here, CP,m is molar heat capacity at constant pressure.

Also, the change in internal energy as follows:

ΔU=CV,mnΔT

Here, CV,m is molar heat capacity at constant volume.

Also,

ΔU=q+w

Here, q is heat and w is work done.

The ideal gas equation is represented as follows:

PV=nRT

Here, P is pressure, V is volume, n is number of moles, R is Universal gas constant and T is temperature.

Answer 12

Expert Solution & Answer

Answer 13

Expert Solution & Answer

Answer 14

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 15

Ch. 5 - Prob. 5.1CP Ch. 5 - Prob. 5.2CP Ch. 5 - Prob. 5.3CP Ch. 5 - Prob. 5.4CP Ch. 5 - Prob. 5.5CP Ch. 5 - Prob. 5.6CP Ch. 5 - Prob. 5.7CP Ch. 5 - Prob. 5.8CP Ch. 5 - Prob. 5.9CP Ch. 5 - Prob. 5.10CP

Want to see the full answer?

Chapter 5 Solutions