2. Consider a particular substance. The isothermal compressibility and coefficient ofthermal expansion are given by:T2K = C1VP2Ta = C3°VPT+ C2VP31+ C4VP2Pa-m3C2 = 2.0Pa2-m3, C3Pa-m31.0Pa2-m3With c, = 0.5K2and c4 = 1.0KKK22a. Determine an exact differential for dV using these two equations. Demonstrate thatthis exact differential does indeed satisfy the Maxwell relations.

Given; κ=c1T2VP2+c2 TVP3α=c3TVP+c41VP2 The equation for isothermal compressibility is;…

2. Consider a particular substance. The isothermal compressibility and coefficient of thermal expansion are given by: T2 K = C1 VP2 T a = C3 VP T + C2 VP3 1 + C4 VP2 With C1 Рa-m3 C2 = Pa2-m3 = 2.0 Ра-m3 ,and c4 K2 Pa2-m3 = 1.0 = 0.5 , C3 = 1.0 K2 K K 2a. Determine an exact differential for dV using these two equations. Demonstrate that this exact differential does indeed satisfy the Maxwell relations.

2. Consider a particular substance. The isothermal compressibility and coefficient of thermal expansion are given by: T2 K = C1 VP2 T a = C3 VP T + C2 VP3 1 + C4 VP2 With C1 Рa-m3 C2 = Pa2-m3 = 2.0 Ра-m3 ,and c4 K2 Pa2-m3 = 1.0 = 0.5 , C3 = 1.0 K2 K K 2a. Determine an exact differential for dV using these two equations. Demonstrate that this exact differential does indeed satisfy the Maxwell relations.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 70AP

See similar textbooks

Similar questions

You have an ideal gas with 1.8 moles. Initally this sample is 187 kPa and 423 K. Heat Capacity at constant presssure is 18.7 J/Kmol. If it undergoed a reversible adiabatic expansion to a temp of 225K. A) what is the final volume? B) what is the final P? C) what is q? D) what is work?
Irreversible Isothermal Compression, Van der Waals Gas Suppose 2.0 mol of CO2(g) undergoes an irreversible isothermal compression at 400 K from 20.0 L to 15.0 L using an external pressure of 30.0 bar. Assume van der Waals gas behavior. For CO2: a = 3.610 atm dm6 mol-2 b = 0.0429 dm3 mol-1 ΔU= ∫ V2 V1 (an^2/V2)dV
Irreversible Isothermal Compression, Van der Waals Gas Suppose 2.0 mol of CO2(g) undergoes an irreversible isothermal compression at 400 K from 20.0 L to 15.0 L using an external pressure of 30.0 bar. Assume van der Waals gas behavior. For CO2: a = 3.610 atm dm6 mol-2 b = 0.0429 dm3 mol-1 ΔU= ∫ V2 V1 (an^2/V2)dV If ΔU = -24 J, what is the numeric value of q (in joules)?
A sample of helium (perfect gas) undergoes a following two-step process.1. Isothermal reversible expansion state 1 (p = 3.0 atm, V = 10.0 L T = 300K) to state 2 (V = 30 L))2. Isobaric compression from state 2 to state 3 (V = 10.0 L) A) What is w and q during step 1? B) What is w and q during step 2? C) What is delta U for the whole process? E) What is delta H for the whole process?
1 kg of benzene is poured into a flask and heated to 353 K (the boiling point of benzeneat 1 atm.) using a heating element that has a power of 700 W (we ignore thatit's probably not so healthy and smart to do). After 5 minutes, when the benzene has stoodboiling point, the heating element is taken up, and the remaining mass of benzene in the flaskmeasured at 470 grams. Determine the enthalpy of vaporization of benzene.
Calculate the isothermal compressibility and isobaric thermal volume expansion from Virial equation in terms of pressure. Virial Equation in terms of pressure: PV = A + Bp + Cp2 + Dp3 + ...
2 moles of water vapor is initially at 400 K. It thermally interacts with 3 moles of a diatomic gas with initial thermal energy of 26500 J. Assume ideal gas behavior and no vibration for both gases. (a). Water molecule has 3 translational and 3 rotational degrees of freedom. What is its Cv? (b). What is the final temperature at thermal equilibrium?
It has been experimentally determined that the heat of combustion of benzene at constant volume is: ΔU ° rxn = -3265.6 kj, at 298K and the heat of combustion at constant pressure is: ΔH ° rxn = -3261.9 kj. C6H6 (l) + 15/2 O2 (g) → 6 CO2 (g) + 3 H2O (l) If we consider that substances in the gas phase behave as ideal gases, responding as appropriate: i) Does the system experience expansion or compression? justify mathematically.
Calculate ∆U and ∆H in heating 55.4 g of Xe from 300 K to 450 K. Assume the heat capacities atconstant volume and constant pressure to be independent of temperature and ideal gas behavior
Calculate the final pressure of a sample of carbon dioxide that expands reversibly and adiabatically from 67.4 kPa and 0.50 dm3 to a final volume of 2.00 dm3. Take γ = 1.4.
Consider an equation of state for a gas given by: ?=1+(?/?? + ?/?2?) where B and C are constants and Z is the compressibility (compression) factor. Derive an expression for the work done in a reversible isothermal expansion from V1 to V2 at temperature T for one mole of the gas.
Suppose an equimolar ideal liquid mixture of A and B initially at 1000C and 200 kPa is isothermally expanded in a cylinder-piston assembly till its starts vaporizing. Determine the pressure at which vaporization starts and the composition of the vapor that forms. The saturation pressures of A and B at 1000C are 120 kPa and 150 kPa, respectively.