Question

Consider the following reaction:

2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g)

The data in the table show the equilibrium constant for this reaction measured at several different temperatures.

Temperature	K
400	1.9x10^7
425	2.5x10^6
465	1.6x10^5
515	8.8x10^3
600	2.0x10^2

Use the data to find ΔrS∘ΔrS∘ for the reaction. (answer in J K-1 mol-1)

The answer is NOT 158

Answer 1

∆S° = -145. 85 J mol-​​​​​​ 1K-1

​​​​​please go through attached images for detailed explan
AG = AGO + 2.3 RT log af AG - Gibbs free energy change Agº – Standard Gibbs free energy R~ gas constant T - Temperature Q – Reaction Quotient. Change at equilibrium, AG=0, & Q = 4 eam constant so, O- Go + 2.3 RT logk logk = -AG° : since DG = BHO_TAS° 2.3RT Togk = - DHO 2.3RT DSO 2.3 R 2.3 RT loqk = -0H + TASO DHO standard enthalpy change standard enkopy Change DS →

@ 400k temperature ko 1:9X16* 8.3 RT log K = -DH + TASO 2.3x8.35 moi' k' x 400 log (19x13) - -H0+ 400 osº 400ko Sº - AH 29,3x8.3 xyoo x7.27 IMO! 400k. Asº - AH = 55513.72 Jmol. eq"O → At book temperatuse k = xX10? y logk = 2 +0.3 = 2.3 6ookos – AH = 2.3 x RT logK 600k, osº -OH = 4.3x8.3Jmo kx 600 K 2.3 Gook. Aso - AH = 26344.20 Jmol ) eqh ® - eq" o Cook. osº - OH = 26344.20 I moi 400k. Osº - anº - 55513.72 I moi) 200k. Aso - - 29 169.52 J moi - 29169.52 Jmoi Ds = 700k os=- 145.85 I mot ky
ation.