### Thermodynamics Exercises**Exercise E3B.3(b)** Estimate the change in the molar entropy of \( \text{N}_2(\text{g}) \) when the temperature is lowered from 298 K to 273 K, given that \( C_{p,m} (\text{N}_2) = 29.125 \, \text{J K}^{-1} \text{mol}^{-1} \) at 298 K.**Exercise E3B.4(a)** The molar entropy of a sample of neon at 298 K is 146.22 J K\(^{-1}\) mol\(^{-1}\). *Note*: The exercises involve calculations related to changes in molar entropy under varying temperature conditions. The given heat capacity \( C_{p,m} \) should be utilized in the calculations for changes in entropy.

Answered: Image /qna-images/answer/67c7fe63-f302-481a-b120-0757743f29f6.jpg

Answered: E3B.3(b) Estimate the change in the…

E3B.3(b) Estimate the change in the molar entropy of N₂(g) when the temperature is lowered from 298 K to 273 K, given that Cpm (N₂) = 29.125 JK' mol¹ at 298 K.

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...

See similar textbooks

Similar questions

(a) An ideal gas of mass 4.5 g and molar mass of 17 g.mole-1 occupies 12.7 L at 310 K. Answer the following questions based on the conditions presented. (i) Calculate the work done under a constant external pressure of 30 kPa until the volume of gas has increased by 3.3 L. (ii) Calculate the work done in an isothermal and reversible expansion process resulting in a final volume of 16L. (iii) If the gas has a molar heat capacity of 30.8 J.mol-1.K-1 and is subjected to a constant volume process until it reaches a temperature of 350K, calculate the heat transfer in kJ.mol-1 of the gas. (b) Calculate the standard enthalpy of formation of N2O5 (g) from N2 (g) and O2 (g), in kJ. mol-1, from the following data: 2NO(g) + O2(g) ® 2NO2(g) DH = -114.1 kJ 4NO2(g) + O2(g) ® 2N2O5(g) DH = -110.2 kJ N2(g) + O2(g) ® 2NO(g) DH = +180.5 kJ
P3B.4 The molar heat capacity of N,(g) in the range 200 K to 400 K is given by Cm/(JK mol) = 28.58 + 3.77 x 10°(T/K). Given that the standard molar entropy of N,(g) at 298 K is 191.6 J Kmol, calculate the value at 373 K. Repeat the calculation but this time assuming that C, is independent of %3D D.m temperature and takes the value 29.13 J K mol. Comment on the difference between the results of the two calculations.
What is the change in (a) the molar internal energy, and (b) the molar enthalpy of a sample of argon gas when it is heated from 273 to 373 K?
Calculate the standard reaction entropy at 298 K of (i) 2 CH3CHO(g) + O2(g) → 2 CH3COOH(l) (ii) 2 AgCl(s) + Br2(l) → 2 AgBr(s) + Cl2(g) (iii) Hg(l) + Cl2(g) → HgCl2(s)
(c) [5 pts] Sketch a graph of the entropy of the van der Waals gas and the entropy of the perfect gas as a function of Vm for b = 1. What happens as b→ 0? Take n = 1 and plot S/nR. (d) [5 pts] Explain the intuition for the graph in (c) using the Boltzmann entropy and the number of microstates.
Half a mole of a perfect gas expands isothermally and at 298.15 K from a volume of 10 L to avolume of 20 L. (a) What is the change in the entropy of the gas? (b) How much work is doneon the gas? (c) What is the heat of Surroundings ? (d) What is the change in the entropy of the surroundings? (e)What is the change in the entropy of the system plus the surroundings?