Chemistry: Atoms First
Chemistry: Atoms First
3rd Edition
ISBN: 9781259638138
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
bartleby

Videos

Textbook Question
Chapter 10.3, Problem 2PPB

(a) Against what external pressure must a gas sample expand from 50.0 mL to 219 mL to do 8.34 J of work? (b) To what volume will a 200.0-mL gas sample be compressed by an external pressure of 7.8 atm if 100.0 J of work are done on the system? (c) To what volume must a 200.0-mL gas sample expand against an external pressure of 7.8 atm to do 100.0 J of work?

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The external pressure and volumes has to be calculated.

Concept Introduction:

At constant pressure, the exchange of heat between the system and surroundings is called as Enthalpy and its state function.

Enthalpy can be given by the formula,

H=U+PV

Where,

H=enthalpy

U=internal energy

P=Pressure

V=Volume

The work done on the system or by the system can be calculated from the equation

w=-PΔV

Where,

w=work done

P=Pressure

V=Change in volume

Answer to Problem 2PPB

The external pressure is 0.487atm .

Explanation of Solution

To calculate the external pressure

Given data:

Initial volume = 50ml

Final volume = 219ml

Change in volume = (219-50)ml=169ml

Work done = 8.34J

w=-PΔV

8.34J=-P(169ml)P=0.0493×1litre.atm101.3JoulesP=0.487atm

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The external pressure and volumes has to be calculated.

Concept Introduction:

At constant pressure, the exchange of heat between the system and surroundings is called as Enthalpy and its state function.

Enthalpy can be given by the formula,

H=U+PV

Where,

H=enthalpy

U=internal energy

P=Pressure

V=Volume

The work done on the system or by the system can be calculated from the equation

w=-PΔV

Where,

w=work done

P=Pressure

V=Change in volume

Answer to Problem 2PPB

The volume is 73.5ml .

Explanation of Solution

To calculate the volume

Given data:

Initial volume = 200 ml

Work done = 100.0J

Pressure = 7.8atm

w=-PΔV

1001litre.atm101.3J=0.987Litre.atm7.8atm=0.981litre.atmChange in volume = 0.9877.8atm=0.1265litresInitialvolume-Finalvolume=0.1265litres0.200litres-Finalvolume=0.1265litresFinalvolume=0.0735litres0.0735litres×1000ml/Litre=73.5ml

Final volume= 73.5ml

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The external pressure and volumes has to be calculated.

Concept Introduction:

At constant pressure, the exchange of heat between the system and surroundings is called as Enthalpy and its state function.

Enthalpy can be given by the formula,

H=U+PV

Where,

H=enthalpy

U=internal energy

P=Pressure

V=Volume

The work done on the system or by the system can be calculated from the equation

w=-PΔV

Where,

w=work done

P=Pressure

V=Change in volume

Answer to Problem 2PPB

The volume is 73.5ml

Explanation of Solution

To calculate the volume

Given data:

Initial volume = 200 ml

Work done = 100.0J

Pressure = 7.8atm

w=-PΔV

1001litre.atm101.3J=0.987Litre.atm7.8atm=0.981litre.atmChange in volume = 0.9877.8atm=0.1265litresInitialvolume-Finalvolume=0.1265litres0.200litres-Finalvolume=0.1265litresFinalvolume=0.0735litres0.0735litres×1000ml/Litre=73.5ml

Final volume= 73.5ml

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Chapter 10 Solutions

Chemistry: Atoms First

Ch. 10.3 - Calculate the work done by or on the system during...Ch. 10.3 - (a) Against what external pressure must a gas...Ch. 10.3 - The diagram on the left shows a sample of gas...Ch. 10.3 - Given the thermochemical equation for...Ch. 10.3 - Calculate the solar energy required to produce...Ch. 10.3 - Prob. 3PPBCh. 10.3 - The diagrams represent systems before and after...Ch. 10.3 - Given the thermochemical equation,...Ch. 10.3 - Given the thermochemical equation,...Ch. 10.4 - Prob. 10.4WECh. 10.4 - Prob. 4PPACh. 10.4 - Prob. 4PPBCh. 10.4 - A metal pellet with a mass of 100.0 g. originally...Ch. 10.4 - What would the final temperature be if the pellet...Ch. 10.4 - Prob. 5PPBCh. 10.4 - Prob. 5PPCCh. 10.4 - A Famous Amos bite-sized chocolate chip cookie...Ch. 10.4 - A serving of Grape-Nuts cereal (5.80 g) is burned...Ch. 10.4 - Prob. 6PPBCh. 10.4 - Suppose an experiment to determine the energy...Ch. 10.4 - Prob. 10.4.1SRCh. 10.4 - Prob. 10.4.2SRCh. 10.4 - Prob. 10.4.3SRCh. 10.4 - Quantities of 50.0 mL of 1.00 M HCl and 50.0 mL of...Ch. 10.5 - Given the following thermochemical equations....Ch. 10.5 - Use the thermochemical equations provided in...Ch. 10.5 - Prob. 10.5.1SRCh. 10.5 - Prob. 10.5.2SRCh. 10.6 - Prob. 10.8WECh. 10.6 - Using data from Appendix 2, calculate Hrn for...Ch. 10.6 - Using data from Appendix 2, calculate Hrn for...Ch. 10.6 - The diagrams represent a system before and after a...Ch. 10.6 - Given the following information, calculate the...Ch. 10.6 - Use the following data to calculate Hf for...Ch. 10.6 - Prob. 9PPBCh. 10.6 - The diagrams represent a system before and after a...Ch. 10.6 - Prob. 10.6.1SRCh. 10.6 - Prob. 10.6.2SRCh. 10.6 - Prob. 10.6.3SRCh. 10.7 - Use bond enthalpies from Table 10.4 to estimate...Ch. 10.7 - Use bond enthalpies from fable 10.4 to estimate...Ch. 10.7 - Prob. 10PPBCh. 10.7 - Prob. 10PPCCh. 10.7 - Prob. 10.7.1SRCh. 10.7 - Prob. 10.7.2SRCh. 10.7 - Prob. 10.7.3SRCh. 10.7 - Prob. 10.7.4SRCh. 10.8 - Prob. 10.11WECh. 10.8 - Prob. 11PPACh. 10.8 - The lattice energy of MgO is 3890 kJ/mol, and the...Ch. 10.8 - Prob. 11PPCCh. 10.8 - Prob. 10.8.1SRCh. 10.8 - Prob. 10.8.2SRCh. 10 - Using data from Appendix 2, calculate the standard...Ch. 10 - Using data from Appendix 2, calculate the standard...Ch. 10 - Prob. 10.3KSPCh. 10 - Prob. 10.4KSPCh. 10 - Define these terms: system, surroundings, thermal...Ch. 10 - What is heat? How does heat differ from thermal...Ch. 10 - Prob. 10.3QPCh. 10 - Define these terms: thermochemistry, exothermic...Ch. 10 - Prob. 10.5QPCh. 10 - Describe two exothermic processes and two...Ch. 10 - Decomposition reactions are usually endothermic,...Ch. 10 - On what law is the first law of thermodynamics...Ch. 10 - Explain what is meant by a state function. Give...Ch. 10 - In a gas expansion, 36 J of heat is absorbed from...Ch. 10 - Prob. 10.11QPCh. 10 - Prob. 10.12QPCh. 10 - Calculate w, and determine whether work is done by...Ch. 10 - Prob. 10.14QPCh. 10 - Prob. 10.15QPCh. 10 - Prob. 10.16QPCh. 10 - Define these terms: enthalpy and enthalpy of...Ch. 10 - Prob. 10.18QPCh. 10 - Prob. 10.19QPCh. 10 - Prob. 10.20QPCh. 10 - Prob. 10.21QPCh. 10 - A gas expands and does PV work on the surroundings...Ch. 10 - Prob. 10.23QPCh. 10 - Prob. 10.24QPCh. 10 - Consider the reaction at a certain temperature. If...Ch. 10 - Prob. 10.26QPCh. 10 - Prob. 10.27QPCh. 10 - Prob. 10.28QPCh. 10 - Prob. 10.1VCCh. 10 - Prob. 10.2VCCh. 10 - Prob. 10.3VCCh. 10 - Prob. 10.4VCCh. 10 - Prob. 10.5VCCh. 10 - Prob. 10.6VCCh. 10 - Prob. 10.7VCCh. 10 - Referring to the process depicted in Figure 10.10,...Ch. 10 - What is the difference between specific heat and...Ch. 10 - Define calorimetry and describe two commonly used...Ch. 10 - A 2.21-kg piece of copper metal is heated from...Ch. 10 - Prob. 10.32QPCh. 10 - A sheet of gold weighing 10.0 g and at a...Ch. 10 - Prob. 10.34QPCh. 10 - A quantity of 2.00 102 mL of 0.862 M HC1 is mixed...Ch. 10 - Prob. 10.36QPCh. 10 - Prob. 10.37QPCh. 10 - Prob. 10.38QPCh. 10 - A 25.95-g sample of methanol at 35.6C is added to...Ch. 10 - Prob. 10.40QPCh. 10 - Prob. 10.41QPCh. 10 - Prob. 10.42QPCh. 10 - Prob. 10.43QPCh. 10 - Prob. 10.44QPCh. 10 - Prob. 10.45QPCh. 10 - Prob. 10.46QPCh. 10 - Prob. 10.47QPCh. 10 - Prob. 10.48QPCh. 10 - Prob. 10.49QPCh. 10 - Prob. 10.50QPCh. 10 - What is meant by the standard-state condition?Ch. 10 - How are the standard enthalpies of an element and...Ch. 10 - What is meant by the standard enthalpy of a...Ch. 10 - Write the equation for calculating the enthalpy of...Ch. 10 - Prob. 10.55QPCh. 10 - Prob. 10.56QPCh. 10 - Prob. 10.57QPCh. 10 - Calculate the heats of combustion for the...Ch. 10 - Calculate the heats of combustion for the...Ch. 10 - Prob. 10.60QPCh. 10 - Prob. 10.61QPCh. 10 - Prob. 10.62QPCh. 10 - From the standard enthalpies of formation,...Ch. 10 - Prob. 10.64QPCh. 10 - Prob. 10.65QPCh. 10 - Prob. 10.66QPCh. 10 - Which is the more negative quantity at 25C: Hf for...Ch. 10 - Prob. 10.68QPCh. 10 - Prob. 10.69QPCh. 10 - Prob. 10.70QPCh. 10 - Prob. 10.71QPCh. 10 - Prob. 10.72QPCh. 10 - Prob. 10.73QPCh. 10 - Prob. 10.74QPCh. 10 - Prob. 10.75QPCh. 10 - Prob. 10.76QPCh. 10 - For the reaction 2C2H6(g)+7O2(g)4CO2(g)+6H2O(g)...Ch. 10 - Prob. 10.78QPCh. 10 - Prob. 10.79QPCh. 10 - Prob. 10.9VCCh. 10 - Prob. 10.10VCCh. 10 - Prob. 10.11VCCh. 10 - Prob. 10.12VCCh. 10 - Explain how the lattice energy of an ionic...Ch. 10 - Specify which compound in each of the following...Ch. 10 - Prob. 10.82QPCh. 10 - Prob. 10.83QPCh. 10 - Prob. 10.84QPCh. 10 - Prob. 10.85QPCh. 10 - Prob. 10.86QPCh. 10 - Prob. 10.87QPCh. 10 - Hydrazine (N2H4) decomposes according to the...Ch. 10 - Prob. 10.89QPCh. 10 - Prob. 10.90QPCh. 10 - Prob. 10.91QPCh. 10 - Prob. 10.92QPCh. 10 - Prob. 10.93QPCh. 10 - Prob. 10.94QPCh. 10 - You are given the following data....Ch. 10 - Prob. 10.96QPCh. 10 - Prob. 10.97QPCh. 10 - Prob. 10.98QPCh. 10 - Prob. 10.99QPCh. 10 - Compare the heat produced by the complete...Ch. 10 - The so-called hydrogen economy is based on...Ch. 10 - Prob. 10.102QPCh. 10 - Prob. 10.103QPCh. 10 - Prob. 10.104QPCh. 10 - Prob. 10.105QPCh. 10 - Prob. 10.106QPCh. 10 - Prob. 10.107QPCh. 10 - Prob. 10.108QPCh. 10 - A certain gas initially at 0.050 L undergoes...Ch. 10 - Prob. 10.110QPCh. 10 - The first step in the industrial recovery of zinc...Ch. 10 - Calculate the standard enthalpy change for the...Ch. 10 - Portable hot packs are available for skiers and...Ch. 10 - Prob. 10.114QPCh. 10 - Prob. 10.115QPCh. 10 - Prob. 10.116QPCh. 10 - Prob. 10.117QPCh. 10 - Prob. 10.118QPCh. 10 - Prob. 10.119QPCh. 10 - Prob. 10.120QPCh. 10 - Prob. 10.121QPCh. 10 - Prob. 10.122QPCh. 10 - Prob. 10.123QPCh. 10 - Prob. 10.124QPCh. 10 - Prob. 10.125QPCh. 10 - Vinyl chloride (C2H3Cl) differs from ethylene...Ch. 10 - Prob. 10.127QPCh. 10 - Prob. 10.128QPCh. 10 - Prob. 10.129QPCh. 10 - Determine the standard enthalpy of formation of...Ch. 10 - Prob. 10.131QPCh. 10 - Prob. 10.132QPCh. 10 - Prob. 10.133QPCh. 10 - Prob. 10.134QPCh. 10 - Prob. 10.135QPCh. 10 - Prob. 10.136QPCh. 10 - Both glucose and fructose arc simple sugars with...Ch. 10 - About 6.0 1013 kg of CO2 is fixed (converted to...Ch. 10 - Experiments show that it takes 1656 kJ/mol to...Ch. 10 - From a thermochemical point of view, explain why a...Ch. 10 - Prob. 10.141QPCh. 10 - Prob. 10.142QPCh. 10 - Prob. 10.143QPCh. 10 - Prob. 10.144QPCh. 10 - Prob. 10.145QPCh. 10 - Prob. 10.146QPCh. 10 - Prob. 10.147QPCh. 10 - Prob. 10.148QPCh. 10 - A drivers manual states that the stopping distance...Ch. 10 - Prob. 10.150QPCh. 10 - Prob. 10.151QPCh. 10 - Prob. 10.152QPCh. 10 - When 1.034 g of naphthalene (C10H8), is burned in...Ch. 10 - Prob. 10.154QPCh. 10 - A gas company in Massachusetts charges 27 cents...Ch. 10 - Prob. 10.156QPCh. 10 - Prob. 10.157QPCh. 10 - According to information obtained from...
Knowledge Booster
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
    Recommended textbooks for you
  • Chemistry
    Chemistry
    ISBN:9781305957404
    Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
    Publisher:Cengage Learning
    Chemistry
    Chemistry
    ISBN:9781133611097
    Author:Steven S. Zumdahl
    Publisher:Cengage Learning
    General Chemistry - Standalone book (MindTap Cour...
    Chemistry
    ISBN:9781305580343
    Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
    Publisher:Cengage Learning
  • Chemistry: The Molecular Science
    Chemistry
    ISBN:9781285199047
    Author:John W. Moore, Conrad L. Stanitski
    Publisher:Cengage Learning
    Chemistry & Chemical Reactivity
    Chemistry
    ISBN:9781133949640
    Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
    Publisher:Cengage Learning
    Chemistry & Chemical Reactivity
    Chemistry
    ISBN:9781337399074
    Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
    Publisher:Cengage Learning
  • Chemistry
    Chemistry
    ISBN:9781305957404
    Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
    Publisher:Cengage Learning
    Chemistry
    Chemistry
    ISBN:9781133611097
    Author:Steven S. Zumdahl
    Publisher:Cengage Learning
    General Chemistry - Standalone book (MindTap Cour...
    Chemistry
    ISBN:9781305580343
    Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
    Publisher:Cengage Learning
    Chemistry: The Molecular Science
    Chemistry
    ISBN:9781285199047
    Author:John W. Moore, Conrad L. Stanitski
    Publisher:Cengage Learning
    Chemistry & Chemical Reactivity
    Chemistry
    ISBN:9781133949640
    Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
    Publisher:Cengage Learning
    Chemistry & Chemical Reactivity
    Chemistry
    ISBN:9781337399074
    Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
    Publisher:Cengage Learning
    The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY