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
Textbook Question
Chapter 4, Problem 4.28E
Can
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Given a thermodynamic function h=h(s,p) show how to evaluate T, V , U , A or F and G
Compute for Delta U,
Delta H and W if 5 moles of an ideal diatomic gas undergoes an isochoric processes (V = k) whose Cv = (5 / 2) R and
Cp = (7/ 2) R from T1 = 273.15 K to T2 = 298.15 K.
The differential for the Gibbs function, G, at constant composition is:
?G = −S?T + Vdp
Using the criterion for exact differentials, write the Maxwell relation that is derived from this equation.
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
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
- A sample consisting of 1.00 mol Ar is expanded isothermally at 20 °C from 10.0 dm3 to 30.0 dm3 (i) reversibly, (ii) against a constant external pressure equal to the final pressure of the gas, and (iii) freely (against zero external pressure). For the three processes calculate q, w, and ΔU.arrow_forwardP2D.2 Starting from the expression Cp − CV = T(∂p/∂T)V(∂V/∂T)p, use theappropriate relations between partial derivatives (The chemist’s toolkit 9 inTopic 2A) to show thatC CT V TV p( / )( / ) p VpT2− = ∂ ∂∂ ∂ Use this expression to evaluate Cp − CV for a perfect gas.arrow_forwardEvaluate (∂S/∂V)T for a van der Waals gas. For an isothermal expansion, will DS be greater for an ideal gas or for a van der Waals gas? Explain your conclusion.arrow_forward
- Calculate 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_forwardA quantity of 0.277 moles of an ideally behaving gas expands isothermally and reversibly from a volume of 5L to twice that volume at 27 ° C. What will be the value of Q, W, ΔU, and ΔH?arrow_forwardProve that P1V1ɣ = P2V2 ɣ for adiabatic reversible events in ideal gases.arrow_forward
- What are ΔS, ΔSsurroundings and Stot for a mole of perfect gas that halves its volume isothermally and reversibly?arrow_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_forwardWhat are ∆S, ∆Sext, ∆Stot for a mole of perfect gas that simultaneously doubles in volume while being compressed and heated to 1000 °C using liquid nitrogen poured onto it by a laser cat? Note that every process is adiabatic and reversible.arrow_forward
- A 2.45 mole quantity of methane gas initially at 315K and a pressure of 12.4atm expands to a final pressure of 0.925atm which is also the constant ext pressure. The expansion occurs adiabatically and reversibly. calculate q, w, deltaH and deltaUarrow_forwardDetermine 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_forwardWhich of the following functions are exact differentials? a dF=1xdx+1ydy b dF=1ydx+1xdy c dF=2x2y2dx+3x3y3dy d dF=2x2y3dx+2x3y2dy e dF=xndx+yndy,n= any integer f dF=(x3cosy)dx+(x3siny)dyarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Physical Chemistry
Chemistry
ISBN:9781133958437
Author:Ball, David W. (david Warren), BAER, Tomas
Publisher:Wadsworth Cengage Learning,
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
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