Thermodynamics, Statistical Thermodynamics, & Kinetics
3rd Edition
ISBN: 9780321766182
Author: Thomas Engel, Philip Reid
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Question
Chapter 3, Problem 3.9NP
Interpretation Introduction
Interpretation:The value of
Concept Introduction:
Different thermodynamic properties like enthalpy, entropy, free energy etc. are used to define different properties like volume, pressure and heat capacity.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
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.7
Calculate V−1(∂V/∂T)p,n for an ideal gas?
Cp− ̄Cv=T ̄V β^2/κ reduces to ̄CP− ̄CV=R for an ideal 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
Similar questions
- A gas obeying the equation of state p(V − nb) = nRT is subjected to a Joule–Thomson expansion. Will the temperature increase, decrease, or remain the same?arrow_forwardThe atomic heat capacity of solid Mo is given by the equation 0.503 x 105 Cp = 5.69 + 1.88 x 10-3 T – T² Find the change in entropy (in eu) which accompanies the heating of one mole of Mo from o C to its melting point, 2620°C. (Entropy unit, (eu) equal to i cal K-¹). Cp expression gives heat capacity in units of cal/mol.arrow_forwardSuppose that a gas obeys at low pressure the equation T + (A + B) P PV = RT + A + where A and Bare constants independent of pressure and temperature, and Vis the molar vo Derive the expression for the change in enthalpy which will accompany the expansion of n moles from a pressure P,to a pressure P, at temperature T. Use this principle. Он OP T T (OT), P = V - Tarrow_forward
- One mol of an ideal gas is heated at a constant external pressure of 200 kPa. Calculate the enthalpy involved and change in internal energy during this process upon the temperature change from 100 oC to 25.0 oC. Molar specific heat capacity CV = 3/2 R and the universal gas constant is 8.3145 J‧mol-1·K-1.arrow_forwardCalculate the change in molar enthalpy DHm when the given gas is heated from 25 oC to 500 oC using the expression above. The constants a, b, and c are available in Table 2B.1.arrow_forwardthe 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 1arrow_forward
- P3A.2 A sample consisting of 0.10 mol of perfect gas molecules is held by a piston inside a cylinder such that the volume is 1.25 dm²; the external is constant at 1.00 bar and the temperature is maintained at 300 Kby a thermostat. The piston is released so that the gas can expand. Calculate (a) the volume of the gas when the expansion is complete; (b) the work done when the gas expands; (c) the heat absorbed by the system. Hence calculate ASor pressurearrow_forwardThe molar heat capacity of a sample of gas at constant-pressure varies with temperature according to the following equation, C_(p,m) (J.K^(-1))=a+bT+c⁄T^2 . Calculate the change in enthalpy of NO(g) when the temperature is raised from 25C to 350C.arrow_forwardCalculate the molar heat capacity at constant pressure (Cp) for a diatomic H2 gas(y = 1.41) with molar heat capacity at constant volume (Cv) of 20.42 J/mol-K?arrow_forward
- Calculate the value of cp at 298 K and 1 atm pressure predicted for Cl, and NO, by the classical equipartition theorem. (Enter your answers to at least two decimal places.) Cp(Cl)) = J mol 1 K1 Cp(NO,) = J mol K1 The actual heat capacities of C and NO, are 33.91 and 36.97 J molK, respectively. Calculate the fraction (expressed as a percentage) of the measured value that arises from vibrational motions. vibrational contribution to cp(Cl,) = vibrational contribution to cp(NO,) =arrow_forwardUse Hess's law to Calculate the AH of the reaction C₂H₂(g) + H₂(g) → C₂H,(g) from the following data. Identify the "manipulation" for each reaction C₂H₂(g) + 3 O₂(g) → 2 CO₂(g) + 2 H₂O(1) C₂H₂(g) + 3% O₂(g) 2 CO₂(g) + 3 H₂O(1) H₂(g) + O₂(g) → H₂O(1) ΔΗ = -1411 kJ AH = -1560 kJ AH = -285.8 kJarrow_forwardRecall that the van der Waals equation of state—an extension of the ideal gas equation—attempts to better capture the behavior of real gases. It can be written to parallel the PV = nRT form of the ideal gas equation: (P + an2/V2) (V − nb) = nRTa) For one mole of a van der Waals gas, derive an expression for the work done by a reversible and isothermal change in volume. In other words, evaluate the following integral for the van der Waals gasw = − {integral with limits from v1 to v2} PdV.b) What are physical interpretations of the van der Waals constants a and b?c) If for helium, the van der Waals constant b is equal to 2.43 × 10–5m3 mol-1, using this value for b, calculate the diameter of the helium atom.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 LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY