Question

03(g) + OH(g) =H(g) + 2 O2(g) AG° = 5.8 kJ/mol at 298 K, A,Gº = 0 kJ/mol at 354 K, and 4 Gº = -2.0 kJ/mol at 373 K. (a) Calculate the equilibrium constant value for this reaction at 298K, 354 K, and 373 K. (b) At 354K, calculate the change in the Gibbs energy of the reaction, AG when the partial pressures of O3 and OH are kept at 10 bar and 30 bar, respectively, while O2 and H have partial pressures of 1.5 bar and 3.0 bar. (c) Based on the conditions corresponding to 1(b), do you expect the reaction to proceed spontaneously?

Answer 1

Saln aiveu Heg2019) Ano kJ/molat 354K -2.0 kJ/mo! at 373 k ohmula Ued R = Q.314 Jwo! k (Gas caustaut) T Teuperature in Keluin) Q Reacton Quohent Here at equilibnum Q K tequilibnium canstcut ) Ar RTl K ANGRTLu K Calulate eguilibnu u caustaut value for tu at 298 K, 354K and 373 K. a) heachon At 29K AG- 5.0 kJ/mol - -8.314 X 290 x k 5000 K 0 096 . at 298 K is o,o96 Hence, eguilibum canstaut

ad 354 K Anй-OкJaol o - RTRn K o, guili biu castaut at 354K 1. 33K A 2.0k/o! at - - & 314 x 373 x Lu K 2000 91 at 373 K So, Esuilibnum custant b) To find change meach on at 354K Partial pressure ol 03 aud 0u are lobar aud sobar wuil 0, aud H have rbar and 2.0ba. RT luQ A ot 8 314 X 354 lu (lb)30) DyG -11167.04 J /mol Ayu 11.17 kJ/no! Ther fore cha i11 KJ/mol 3 Kis tea conditiou corespaudiug to 1 b) to phocsed spantaueousy C Yes, based on conty нeachim Tne