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 5, Problem 5.5NP
Interpretation Introduction
Interpretation:
The value of change in entropy for the given transformation needs to be determined.
Concept Introduction :
The entropy of a system is defined as degree of randomness in the system.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
The equilibrium constant of the reaction 2 X (g) = Y (g) + Z(g) is found to fit the expression lnK = A + B/T + C/T2 between 300K and 600K, with A = 1.09, B = 1003K and C = 1.46 x 105 K2. Calculate the standard reaction entropy, J K-1mol-1, at 338K. 2 decimal.
At 25 °C, the equilibrium partial pressures for the reaction
2 A(g) + 4B(g)2C(g) + D(g)
were found to be P = 5.98 bar, P = 4.72 bar, Pe= 5.25 bar, and P = 4.16 bar.
What is the standard change in Gibbs free energy of this reaction at 25 °C?
AGOR=
kJ/mol
The change in the Gibbs energy of a certain constant-pressure process was found to fit the expression ΔG/J = −73.1 + 42.8(T/K). Calculate the value of ΔS for the process, and please explain what happened to ΔH along the way.
Chapter 5 Solutions
Thermodynamics, Statistical Thermodynamics, & Kinetics
Ch. 5 - Under what conditions is S0 for a spontaneous...Ch. 5 - Why are Sfustion and Svaporization always...Ch. 5 - An ideal gas in thermal contact with the...Ch. 5 - Prob. 5.4CPCh. 5 - Prob. 5.5CPCh. 5 - You are told that S=0 for a process in which the...Ch. 5 - Under what conditions does the equality S=H/T...Ch. 5 - Is the following statement true or false? If it is...Ch. 5 - Prob. 5.9CPCh. 5 - One Joule of work is done on a system, raising its...
Ch. 5 - Prob. 5.11CPCh. 5 - An ideal gas undergoes an adiabatic expansion into...Ch. 5 - When a saturated solution of a salt is cooled, a...Ch. 5 - Prob. 5.14CPCh. 5 - Prob. 5.15CPCh. 5 - Prob. 5.16CPCh. 5 - Why is the efficiency of a Carnot heat engine the...Ch. 5 - Two vessels of equal volume, pressure and...Ch. 5 - Solid methanol in thermal contact with the...Ch. 5 - Can incandescent lighting be regarded as an...Ch. 5 - The Chalk Point, Maryland, generating station...Ch. 5 - An electrical motor is used to operate a Carnot...Ch. 5 - An air conditioner is a refrigerator with the...Ch. 5 - Prob. 5.5NPCh. 5 - The average heat evolved by the oxidation of...Ch. 5 - Prob. 5.9NPCh. 5 - The maximum theoretical efficiency of an internal...Ch. 5 - Prob. 5.11NPCh. 5 - Prob. 5.12NPCh. 5 - Prob. 5.13NPCh. 5 - Prob. 5.14NPCh. 5 - Prob. 5.15NPCh. 5 - Prob. 5.16NPCh. 5 - Prob. 5.17NPCh. 5 - Prob. 5.18NPCh. 5 - Prob. 5.19NPCh. 5 - Prob. 5.20NPCh. 5 - Prob. 5.21NPCh. 5 - Prob. 5.22NPCh. 5 - Prob. 5.23NPCh. 5 - Prob. 5.24NPCh. 5 - Prob. 5.25NPCh. 5 - Prob. 5.26NPCh. 5 - Under anaerobic conditions, glucose is broken down...Ch. 5 - Prob. 5.28NPCh. 5 - Prob. 5.29NPCh. 5 - Prob. 5.30NPCh. 5 - Prob. 5.31NPCh. 5 - Calculate Ssurroundings and Stotal for the...Ch. 5 - A refrigerator is operated by a 0.25-hp...Ch. 5 - Prob. 5.34NPCh. 5 - Between C and 100C, the heat capacity of Hg(l) is...Ch. 5 - Prob. 5.36NPCh. 5 - Prob. 5.37NPCh. 5 - Prob. 5.38NPCh. 5 - Prob. 5.39NPCh. 5 - Prob. 5.40NPCh. 5 - Prob. 5.41NPCh. 5 - Prob. 5.42NPCh. 5 - An ideal gas sample containing 1.75 moles for...Ch. 5 - Prob. 5.44NPCh. 5 - Prob. 5.45NP
Knowledge Booster
Similar questions
- The equilibrium constant for a chemical reaction was found to depend on temperature over the temperature range 400 K to 600 K according to the following equation:ln K(T) = A +BT+CT2where A, B, and C are the constants A = −3.53, B = −2736 K, and C = 2.2 × 105 K2.Calculate the standard reaction enthalpy and the standard reaction entropy at T =500 K.arrow_forwardCalculate ΔS (for the system) when the state of 2.00 mol of gas molecules, for which Cp,m = 7/2 R, is changed from 25 °C and 1.50 atm to 135 °C and 7.00 atm.arrow_forwardAt 25 °C, the equilibrium partial pressures for the reaction 2 A(g) + 4 B(g)=2C(g)+D(g) were found to be PA = 4.74 bar, Pg 5.52 bar, Pc = 4.94 bar, and Pp 5.78 bar. What is the standard change in Gibbs free energy of this reaction at 25 °C? ?arrow_forward
- At 25 °C, the equilibrium partial pressures for the reaction 2A(g)+4B(g)↽−−⇀2C(g)+D(g) were found to be PA=5.86 bar, PB=5.73 bar, PC=4.88 bar, and PD=4.65 bar. What is the standard change in Gibbs free energy of this reaction at 25 °C? ΔGrxn°= kJ/molarrow_forwardThe equilibrium constant of the reaction 2 C3H6(g) ⇋ C2H4(g) + C4H8(g) is found to fit the expression ln K = A + B/T + C/T2 between 300 K and 600 K, with A = −1.04, B = −1088 K, and C = 1.51 × 105 K2. Calculate the standard reaction enthalpy and standard reaction entropy at 400 K.arrow_forwardAt 25 °C, the equilibrium partial pressures for the reaction 2 A(g) + 4B(g) = 2C(g) + D(g) were found to be P = 4.62 bar, P = 4.70 bar, Pe=5.81 bar, and Pp = 5.90 bar. What is the standard change in Gibbs free energy of this reaction at 25 C? AG kJ/molarrow_forward
- The change in the Gibbs energy of a certain constant-pressure process is found to fit the expression ΔG/J = −85.40 + 36.5(T/K). Use the Gibbs–Helmholtz equation to calculate the value of ΔH for the process.arrow_forwardThe standard molar entropy of benzene is 173.3 J K-1 mol-1. Calculate the change in its standard molar Gibbs energy when benzene is heated from 25°c to 45 °c.arrow_forwardThe equilibrium constant of a reaction is found to fit the expression ln K = A + B/T + C/T3 between 400 K and 500 K with A = −2.04, B = −1176 K, and C = 2.1 × 107 K3. Calculate the standard reaction enthalpy and standard reaction entropy at 450 K.arrow_forward
- Given that the Gibbs energy is a function of temperature and pressure G(T, P), estimate the change in molar Gibbs energy (AGm) of methanol at 298.15 K when the external pressure increases from 1.00 bar to 1.25 bar. At 298.15 K, the density (p) of methanol is 0.792 g/cm² and the molar entropy (Sm) of methanol is 126.8 J mol·' K'. A. AGm S -10“ J B. -10* J < AG, 3 -10³ J C. -10' J < AGm < -100 J D. -100 J < AGm S -10 J E. -10 J < AGm s -1.0 J F. -1.0 J < AGm s 0J G. 0J < AGm s 1.0 J H. 1.0 J < AGm < 10 J I. 10 J < AGm s 100 J J. 100 J < AGm < 10³ J K. 10 J < AGm s 10ª J L. 104 J < AGmarrow_forwardAccording to the table of the molecule in two temperatures points T(K) Kd 273.15 1,32 x 10-10 320.15 3,44 х 109 Calculate the standard (molar) entropy of dissociation of this molecule at 273.15 K, assuming that the standard (molar) dissociation enthalpy can be considered as constant between 273.15 K and 320.15 K. Where (Kd) is the dissociation constant and T(K) are temperatures in Kelvin.arrow_forwardEstimate the enthalpy of reaction h̄R for the dissociation process CO2 ⇌ CO + 1⁄2 O2 at 2200 K, using (a) enthalpy data and (b) KP data.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning