B4.Use the data below to calculate the equilibrium constant at 1000 K for the reaction 2Hlg)→H2e+l2e △H°kJmo) S(J mol) 26.5 206.6 H2xg) 0.0 130.6 12g0 62.4 260.7 △H°=△H'Hg)+△HI2g）-2△H'(Hg) =0+62.4-2(26.5)=9.4 kJ mol △S°=△Sr'Hg)+△SrL2g）-2△Sr'Hlg) =130.6+260.7-2(206.6)=-21.9JKmo △G°=△H°.TAS9 =9400-1000(-21.9=+31,300Jmor K-d0.em0023 (b)If p=0.002 atm at equilibrium,calculate Pe and pr2. PnP=0.023 P p,P,=0.023p=0.023(0.002atm)2=9.27×10-8atm Thus,p4,=P2=(9.27×108atm2)v2=3.04×10atm B5.(a)What hybridization is each of the four indicated atoms using in the molecule of Aspirin shown below? 5 B4. Use the data below to calculate the equilibrium constant at 1000 K for the reaction 2 HI(g) → H2(g) + I2(g) ΔHf o (kJ mol-1) So (J mol-1) HI(g) 26.5 206.6 H2(g) 0.0 130.6 I2(g) 62.4 260.7 ΔHo = ΔHf 0 (H2(g)) + ΔHf 0 (I2(g)) – 2 ΔHf 0 (HI(g)) = 0 + 62.4 – 2(26.5) = 9.4 kJ mol-1 ΔSo = ΔSf 0 (H2(g)) + ΔSf 0 (I2(g)) – 2 ΔSf 0 (HI(g)) = 130.6 + 260.7 – 2(206.6) = –21.9 J K-1 mol-1 ΔGo = ΔHo - TΔSo = 9400 – 1000(-21.9) = +31,300 J mol-1 0 1 1 1 G 31300 Jmol RT 8.314 JK mol (1000K) Ke e 0.023 − − − ⎡⎤ ⎡ −Δ − ⎤ ⎢⎥ ⎢ ⎥ ⎢⎥ ⎢ ⎣⎦ ⎣ ⎥⎦ == = (b) If pHI = 0.002 atm at equilibrium, calculate pH2 and pI2. 2 2 2 2 H I 2 HI 2 2 H I HI p p 0.023 p p p 0.023p 0.023(0.002atm) 9.27 10 atm − = = = =× 8 2 Thus, 2 2 8 2 1/ 2 4 p p (9.27 10 atm ) 3.04 10 atm H I − − == × = × B5. (a) What hybridization is each of the four indicated atoms using in the molecule of Aspirin shown below? 5