Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
expand_more
expand_more
format_list_bulleted
Question
Chapter 4, Problem 4.71E
Interpretation Introduction
(a)
Interpretation:
Whether the chemical potential of
Concept introduction:
The chemical potential is the energy absorbed or released in a
Interpretation Introduction
(b)
Interpretation:
Whether the chemical potential of
Concept introduction:
The chemical potential is the energy absorbed or released in a chemical reaction or in phase transition. Chemical potential shows the change in Gibbs function with the change in composition of mixture.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
(a) From the phase diagram for carbon dioxide, determine the state of co2 at 20 atm and 273 K.
(b) Explain why co2 can undergo sublimation under normal condition.
The 1980s saw reports of ΔfH⦵(SiH2) ranging from 243 to 289 kJ mol−1. If the standard enthalpy of formation is uncertain by this amount, by what factor is the equilibrium constant for the formation of SiH2 from its elements uncertain at (a) 298 K, (b) 700 K?
Indicate whether each of the following statements is true orfalse. If it is false, correct it. (a) The feasibility of manufacturingNH3 from N2 and H2 depends entirely on the valueof ΔH for the process N2(g) + 3 H2(g)----->2 NH3(g).(b) The reaction of Na(s) with Cl2(g) to form NaCl(s) is aspontaneous process. (c) A spontaneous process can in principlebe conducted reversibly. (d) Spontaneous processes ingeneral require that work be done to force them to proceed.(e) Spontaneous processes are those that are exothermicand that lead to a higher degree of order in the system.
Chapter 4 Solutions
Physical Chemistry
Ch. 4 - List the sets of conditions that allow dS, dU, and...Ch. 4 - Explain why conditions for using S>0 as a strict...Ch. 4 - Explain how the equation dU+pdVTdS0 is consistent...Ch. 4 - Explain why the spontaneity conditions given in...Ch. 4 - Prove that the adiabatic free expansion of an...Ch. 4 - Derive equation 4.6 from equation 4.5.Ch. 4 - Derive equation 4.8 from equation 4.7.Ch. 4 - The third part of equation 4.9 mentions a...Ch. 4 - Calculate A for a process in which 0.160mole of an...Ch. 4 - What is the maximum amount of non-pV work that can...
Ch. 4 - Consider a piston whose compression ratio is 10:1;...Ch. 4 - When one dives, water pressure increases by 1atm...Ch. 4 - Calculate G(25C) for this chemical reaction, which...Ch. 4 - Thermodynamic properties can also be determined...Ch. 4 - Calculate G in two different ways for the...Ch. 4 - Calculate G in two different ways for the...Ch. 4 - For the reaction C(graphite)C(diamond) at 25C,...Ch. 4 - Determine G for the following reaction at 0C and...Ch. 4 - What is the maximum amount of electrical that is,...Ch. 4 - When a person performs work, it is non-pV work....Ch. 4 - Can non-pV work be obtained from a process for...Ch. 4 - Can pV work be obtained from a process for which...Ch. 4 - Batteries are chemical systems that can be used to...Ch. 4 - The value of G for any phase change at constant p...Ch. 4 - The value of G for any phase change at constant p...Ch. 4 - Under what conditions is A=0 for a phase change?...Ch. 4 - Example 4.2 calculated A for one step of a Carnot...Ch. 4 - Can CV and Cp be easily defined using the natural...Ch. 4 - Analogous to equation 4.26, what is the expression...Ch. 4 - Prob. 4.30ECh. 4 - Prob. 4.31ECh. 4 - Prob. 4.32ECh. 4 - Although ideally, U=H=0 for a gas-phase process at...Ch. 4 - Use equations 4.21 and 4.25 to explain why H and G...Ch. 4 - Prob. 4.35ECh. 4 - Which of the following functions are exact...Ch. 4 - Prob. 4.37ECh. 4 - Prob. 4.38ECh. 4 - Prob. 4.39ECh. 4 - Equation 4.19 says that (UV)S=p If we are...Ch. 4 - For an isentropic process, what is the approximate...Ch. 4 - Use the ideal gas law to demonstrate the cyclic...Ch. 4 - Prob. 4.43ECh. 4 - Prob. 4.44ECh. 4 - Evaluate (U/V)T for an ideal gas. Use the...Ch. 4 - Evaluate (U/V)T for a van der Waals gas. Use the...Ch. 4 - Repeat the previous exercise for a gas that...Ch. 4 - Determine an expression for (p/S)T for an ideal...Ch. 4 - Determine the value of the derivative {[(G)]/T}p...Ch. 4 - Prob. 4.50ECh. 4 - Prob. 4.51ECh. 4 - A 0.988-mole sample of argon expands from 25.0L to...Ch. 4 - A 3.66-mol sample of He contracts from 15.5L to...Ch. 4 - Prob. 4.54ECh. 4 - Prob. 4.55ECh. 4 - Use the Gibbs-Helmholtz equation to demonstrate...Ch. 4 - For the equation 2H2(g)+O2(g)2H2O(g)...Ch. 4 - Use equation 4.46 as an example and find an...Ch. 4 - What is the value of G when 1.00mol of water at...Ch. 4 - Prob. 4.60ECh. 4 - Prob. 4.61ECh. 4 - Prob. 4.62ECh. 4 - Prob. 4.63ECh. 4 - Prob. 4.64ECh. 4 - What is the change in the chemical potential of a...Ch. 4 - Prob. 4.66ECh. 4 - Prob. 4.67ECh. 4 - Prob. 4.68ECh. 4 - Prob. 4.69ECh. 4 - Can equation 4.62 be used to calculate for an...Ch. 4 - Prob. 4.71ECh. 4 - Of helium and oxygen gases, which one do you...Ch. 4 - Prob. 4.73ECh. 4 - Use equation 4.39 to determine a numerical value...Ch. 4 - Prob. 4.75ECh. 4 - Prob. 4.76E
Knowledge Booster
Similar questions
- Data are given in Appendix 1 for white phosphorus, P4(s). P4(g) has the following thermodynamic values: Hf=58.9kJ/mol , S=280.0J/kmol . What is the temperature at which white phosphorus sublimes at 1 atm pressure?arrow_forwardThe phase diagram for SO2 is shown here. (a) What doesthis diagram tell you about the enthalpy change in thereaction SO2(l) ---->SO2(g)? (b) Calculate the equilibriumconstant for this reaction at 100 °C and at 0 °C.(c) Why is it not possible to calculate an equilibrium constantbetween the gas and liquid phases in the supercriticalregion? (d) At which of the three points marked in reddoes SO2(g) most closely approach ideal-gas behavior?(e) At which of the three red points does SO2(g) behaveleast ideally?arrow_forward6. When the ideal-gas reaction A+B=C+Dhas reached equilibrium, state whether or not each of the following relations must be true. Here n¡ is the number of moles of species i in equilibrium, P, is the partial pressure of i, and µ; is the chemical potential of i. Here a simple True or False answer is sufficient. (a) nc+np=nA +ng (b) Pc+Pp=PA+PB (c) na=ng (d) nc=na (e) If only A and B are present initially, then nc=np (f) Ha + HB= Hc+ Hp no matter what the initial composition. (g) If only A and B are present initially, then in equilibrium we must have nc # 0. (h) The equilibrium constant Kp(T)= PĄPB/(PcPp). (i) The value of –RT In Kp(T) = µE(T)+µ8(T)– H3(T) –- H§(T). ) The equilibrium constant is independent of the total pressure.arrow_forward
- Iron is heated from 100 °C to 1000 °C. By how much does its chemical potential change (kJ)? Take Sm° = 53 J K1 mol·1 for the entire range. Larrow_forwardGiven that AG; for NH3 = -16.666 kJ/mol, calculate the equilibrium constant for the following reaction at 298 K: N2(g) + 3H2(g) = 2NH3(g) 6.96 x 105 O 1.01 O 4.43 x 1069 5.81 x 108 8.34 x 102arrow_forwardWrite the formula for hypoiodous acid. formula: || SPECIAL ΔΣΩ λμπ x" Xo x (s) (1) (aq) (g) () [] CLRarrow_forward
- (a) Given the ionic radii, Cst = 1.67Å, CI = 1.81Å, and the Madelung constant M(CSCI) = 1.763, determine to the best of your ability the molar Crystal energy (AEcryst) for CsCl. (b) Not given additional data, do you expect the value obtained to be larger or smaller than theoretical, and by how many percent do you anticipate to be off?arrow_forwardConsider the following reaction at 25°C: 3 Ni(s) + N²(g) + 3 H2O(g) → 3 NiO(s) + 2NH:(g) where K = 6.74 x 104 At what partial pressure of ammonia will one be able to get out 11.5 kJ/mol of Gibbs free energy from this reaction when the rest of the mixture contains 57.6 g NiO, 182.3 g Ni, 8.54 atm of nitrogen gas, and 10.07 atm of water vapor? (Enter the partial pressure using two significant figures.)arrow_forwardCalculate the standard Gibbs free energy in kJ mol–1.arrow_forward
- 8. (a) The enthalpy of the fusion of metal Cesium is 13.5 kJ/mol at the melting point of 28.5 oC. Calculate the entropy change for Cesium going from solid to liquor.arrow_forward(a) The equilibrium constant of the isomerization of cis-2-butene to trans-2-butene is 2.07 at 127.0 °C. Determine the standard molar Gibbs free energy, AGR º for the reaction. (b) For C6o, the standard molar Gibbs free energy (AG, º) of formation from the elemental carbon is 23.98 kJ/mol at 25.0 °C. Determine the equilibrium constant, Keq for the formation of C60.arrow_forwardHydrogen peroxide can be prepared in several ways. One method is the reaction between hydrogen and oxygen, another method is the reaction between water and oxygen. Calculate the AGxn of each reaction using values from the table of thermodynamic properties. (1) H,(g) +0,(g) =H,0,1) AGan = kJ-mol- (2) H,O() + 0,(g) 2H,0,(1) kJ-mol AGn = Which method requires less energy under standard conditions? O reaction (1) reaction (2) Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Refer to the AG, values. 3H,(g) + Fe,0,(s) – - 2 Fe(s) + 3 H,0(g) AG°an = kJarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher: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