Obtain an expression for the isobaric volumetric thermal expansion coefficient 1 (m) for an ideal gas. Work has to be shown. Based on your result, do you expect a for Vm OT an ideal gas to be always positive, always negative, or that it depends on conditions? Explain. α

Obtain an expression for the isobaric volumetric thermal expansion coefficient 1 (m) for an ideal gas. Work has to be shown. Based on your result, do you expect a for Vm OT an ideal gas to be always positive, always negative, or that it depends on conditions? Explain. α

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Obtain an expression for the isobaric volumetric thermal expansion coefficient 1 (m) for an ideal gas. Work has to be shown. Based on your result, do you expect a for Vm OT an ideal gas to be always positive, always negative, or that it depends on conditions? Explain. α
(a) Suppose that attractions are the dominant interaction between gas molecules, and the equation of state is p = nRT/V – n2a/V2. Determine the work (W(non-ideal gas)) of reversible, isothermal expansion of such a gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol, T = 300 K, and a = 3.621 atm-L2/mol2. Watch your units. (b)Determine the work (W(ideal gas) of reversible, isothermal expansion of an ideal gas from initial volume V (initial) = 20.0 L to final volume V(final) = 40.0 L if n = 2.00 mol and T = 300 K. (c) Show the difference W(non-ideal) – W(ideal). If all your calculations are done correctly, this result shows you the effect of attractive interaction between gas particles on the work done by the system.
Calculate delta G for the isothermal expansion of 3.75 mol of an ideal gas at 315 K from an intial pressure of 1.15x10^6 Pa to a final pressure of 5.40x10^3 Pa.
5. A sample consisting of 3 mol of ideal gas molecules with Cp.m = 20.8 J K-1 mol-1 is initially at 240 kPa and 325 K. It undergoes reversible adiabatic expansion until its pressure reaches 150 kPa. Calculate (i) the final volume and temperature, (ii) q, (iii) w, and (iv) AU.
1) A sample containing 1.50 mol of an ideal gas with CV,m = 20.8 J K−1 mol−1isinitially at 230 kPa and 315 K. It undergoes a reversible adiabatic expansion until itspressure reaches 170 kPa. Calculate the final volume V2; the final temperature T2, andthe work w done by the system.
B1. Prove that for a 1 component Ideal Gas: G(T,P2,n) = G(T,P1, n) + nRT In