Question

Please explain as much as possible. Why did you use the equation? Or what conditions did you see from the question? etc.

a) Show that the molar entropy change, ASm, is given by ASm Cym In2 Rln if one mole of an ideal gas is taken from T, , V to T2 , V2 assuming that Cy m is independent of temperature. b) Calculate the value of the molar entropy change, AS,m, if one mole of N2(g) is expanded from 20.0 dm2 at 273 K to 300 dm3 at 400 K. (Cp,m 29.4J K-1mol-1)

Answer 1

$\Delta S=(21.086*0.38+8.314*2.708)J/K$

by definchon of entrópy As = 9rev Allure que he per absorbed To Temperature from 1st Law of thermodynamics au = &ver + When 14 - w - Prev All thodu = Eren dinding bein side by at . het en av = alogue : 45. work done -P du Prey At constant volume cv = (du) (vdt) - du Cv att l dv = 15 17 T thing ideal gas equ .PV = nRT for 1 mole fr=RT C & de + edr = as & substituting this in phone substituting this in alove ( 9 " Z vyk as, to AS, G mit te ihny cu into tR in 4 zos = 15) (Assumed 'co independent 8 temperature = 24.4Jkt mot ſwe know -tvaror & Boa Imole a ix ev = 21.086 Jk"). CD-R =(29.4-8-314)J *o 7 21.086 Jkt met 7 T = 273k v. = 20 dm3 45 - 21.086 I 400 5: Ar kv + 18 500 dim. Scanned with 28737 45. ns21.9864 0.38 +8.314 2.708

$\Delta S=(8.01268+22.51) J/K$

$\Delta S=30.522J/K$