Thermodynamics, Statistical Thermodynamics, & Kinetics
3rd Edition
ISBN: 9780321766182
Author: Thomas Engel, Philip Reid
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 3, Problem 3.13NP
Interpretation Introduction
Interpretation:
From equation
Concept Introduction :
The relationship between Cp and Cv with
is represented as follows:
Here, Cp is the specific heat capacity at constant pressure, Cv is the specific heat capacity at constant volume, T is temperature, V is volume,
and
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
the ionic compound L2O3(s) is the ionic compound formed from oxygen and a metal
with the form L(s) at 1.00 bar and 298 K.
(a) Draw the Lewis structure for L2O3. Assume that all the valence electrons from L
are required.
(b) Use the following information to determine the enthalpy of formation for
L2O3(s). Express your answer in kJZ(mol L2O3(s)).
Lattice energy for L2O3(s) = -14836 kJ mol1
AHsub for L(s) = 358 kJ mol 1
First ionization energy for L(g) = 577 kJ mol 1
Second ionization energy for L(g) = 1794 kJ mol 1
Third ionization energy for L(g) = 3820 kJ mol 1
Bond dissociation energy for O2(g) = 498 kJ mol 1
%3D
First electron affinity for O = -141 kJ mol 1
Second electron affinity for O = 744 kJ mol 1
One mole (1.0 mol) of an ideal gas is initially at T1 = 298 K and has volume V1 = 2.0 L. It is then reversibly expanded to final volume V2 = 3.0 L. Assume Cp = 5/2 R and Cv = 3/2R.
a) Calculate the following if the expansion is isothermal: 1) ΔT
2) q
3) w 4) ΔU
5) ΔH
b) Calculate ΔT–ΔU if the expansion is adiabatic instead of isothermal.c) Calculate the initial pressure and two final pressures for the process in a) & b).d) On a single set of axes, sketch a pressure–volume plot for each of the two processes in a) & b). Label the area that corresponds to the work for each process.
Assume N₂ behaves as perfect gas. It expands reversibly and adiabatically from Vi to Vf with the pressure change from pi to pf.
(a) Derive the temperature versus volume relationship and the pressure and volume relationship for this expansion.
(b) When a sample of N₂ of mass 3.12 g at 23.0 °C is allowed to expand reversibly and adiabatically from 4.00 × 10² cm3 to 2.00 dm3, what is the work done by the gas?
Chapter 3 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
Ch. 3 - Prob. 3.1CPCh. 3 - Prob. 3.2CPCh. 3 - Prob. 3.3CPCh. 3 - Prob. 3.4CPCh. 3 - Why can qv be equated with a state function if q...Ch. 3 - Prob. 3.6CPCh. 3 - Prob. 3.7CPCh. 3 - Prob. 3.8CPCh. 3 - Prob. 3.9CPCh. 3 - Why is qv=U only for a constant volume process? Is...
Ch. 3 - Prob. 3.11CPCh. 3 - Why are q and w not state functions?Ch. 3 - Prob. 3.13CPCh. 3 - What is the relationship between a state function...Ch. 3 - Prob. 3.15CPCh. 3 - Is the following statement always, never, or...Ch. 3 - Is the following statement always, never, or...Ch. 3 - Prob. 3.18CPCh. 3 - Prob. 3.19CPCh. 3 - Is the expression UV=T2T1CVdT=nT1T2CV,mdT only...Ch. 3 - Prob. 3.1NPCh. 3 - Prob. 3.2NPCh. 3 - Prob. 3.3NPCh. 3 - Prob. 3.4NPCh. 3 - Prob. 3.5NPCh. 3 - Prob. 3.6NPCh. 3 - Integrate the expression =1/VV/TP assuming that ...Ch. 3 - Prob. 3.8NPCh. 3 - Prob. 3.9NPCh. 3 - Prob. 3.10NPCh. 3 - Prob. 3.11NPCh. 3 - Calculate w, q, H, and U for the process in which...Ch. 3 - Prob. 3.13NPCh. 3 - Prob. 3.14NPCh. 3 - Prob. 3.15NPCh. 3 - Prob. 3.16NPCh. 3 - Prob. 3.17NPCh. 3 - Prob. 3.18NPCh. 3 - Prob. 3.19NPCh. 3 - Prob. 3.20NPCh. 3 - Prob. 3.21NPCh. 3 - Prob. 3.22NPCh. 3 - Derive the following relation, UVmT=3a2TVmVm+b for...Ch. 3 - Prob. 3.24NPCh. 3 - Prob. 3.25NPCh. 3 - Prob. 3.26NPCh. 3 - Prob. 3.27NPCh. 3 - Prob. 3.28NPCh. 3 - Prob. 3.29NPCh. 3 - Prob. 3.30NPCh. 3 - Prob. 3.31NPCh. 3 - Prob. 3.32NPCh. 3 - Prob. 3.33NPCh. 3 - Prob. 3.34NPCh. 3 - Derive the equation H/TV=CV+V/k from basic...Ch. 3 - Prob. 3.36NPCh. 3 - Prob. 3.37NPCh. 3 - Show that CVVT=T2PT2VCh. 3 - Prob. 3.39NP
Knowledge Booster
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
- In the equation w = P V, why is there a negative sign?arrow_forwardUse the data in Table 2.2 to determine Hp T for Ar at 0C and 1atm. Make any reasonable assumptions necessary.arrow_forwardWhat is the change in internal energy when a gas contracts from 377mL to 119mLundera pressure of 1550 torr, whileat the same time being cooled by removing 124.0J ofheat energy?arrow_forward
- Determine an expression for V/T p, n in terms of and . Does the sign on the expression make sense in terms of what you know happens to volume as temperature changes?arrow_forwardAt the critical point for carbon dioxide, the substance is very far from being an ideal gas. Prove this statement by calculating the density of an ideal gas in g/cm3 at the conditions of the critical point and comparing it with the experimental value. Compute the experimental value from the fact that a mole of CO2 at its critical point occupies 94 cm3.arrow_forward11. For a certain ideal gas, the increase of enthalpy is 34 Kcal when the pressure increases from 0.11 MPaa to 1.1 MPaa and the volume increases from 12.6 gallons to 19.7gallons. Determine (a) AU and (b) T₂ if T₁ = 303 K.arrow_forward
- What if we assumed that the heat capacity of gaseous NH3 is NOT dependent on temperature? Calculate the energy per mole required to be removed from gaseous NH3 from decrease the temperature of the system from 400 °C to 25 ºC. Assume that the heat capacity, Cpm, of NH3 is a constant over the temperature range considered and can be found in Table 2C.7arrow_forwardOne mole (1.0 mol) of an ideal gas is initially at T1 = 298 K and has volume V1 = 2.0 L. It is then reversibly expanded to final volume V2 = 3.0 L. Assume Cp = 5/2 R and Cv = 3/2R. a) Calculate the following if the expansion is adiabatic: 1) ΔT 2) q 3) w 4) ΔU 5) ΔHarrow_forwardCalculate V−1(∂V/∂T)p,n for an ideal gas?arrow_forward
- One mole of N2(g) occupies 5 L of volume at 300 K in a sealed cylinder. The gas behaves ideally in expanding isothermally to 10 L. Calculate w, ΔE and ΔH if the expansion proceeds (i) reversibly, (ii) irreversibly against an external pressure at 0.2 atm.arrow_forward4. The heat capacity of solid lead oxide is given by the equation: Cp(T) = 44.35 + 1.47 × 10-3 xT with T in units of K and the resulting Cp(T) in units of K-mol Calculate the change in enthalpy of 1 mole of PbO(s) if it is heated from 200 to 600 K at constant pressure. (Assume no phase transitions take place during this process.)arrow_forwardThe temperature dependence of the molar heat capacity cp of nitrogen can be written as: Ср c₂ = (27.27 +5.22-10³ T/K – 0.0042·10° T²³/K²) J/(K·mol). Calculate the required heat to increase the temperature at constant volume of 1mol N₂ from 273 to 1273 K (mind the difference between c, and c₁).arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning