(2)Partial pressure equilibrium constants K1P"PHKPPP:Pa
(2) Partial pressure equilibrium constants Kp Kp = b B a A h H g G P P P P P：Pa
(3)HeterogeneousequilibiumCaCO;(s) = CaO(s) + CO,(g)K,= [CO2]K,=Pco2CaCO3(s) + H,O (l) + CO2(g) =Ca2+ (aq)+ 2HCO3(aq)
(3) Heterogeneous equilibium CaCO3 (s) = CaO(s) + CO2 (g) Kc = [CO2 ] Kp = P CO2 CaCO3 (s) + H2O (l) + CO2 (g) = Ca2+ ( aq)+ 2HCO3 - (aq)
2.2.2 Standard equlibrium constants[(][G][H]Co(a+b)-(g+h)(1)In solution,K=[A][B](()()()= K, · Po(a+b)-(g+h)(2)Ingasphase,Ko(X)
2.2.2 Standard equlibrium constants (1) In solution, Kº= (a b) (g h) a b g h a b g h C A B G H C B C A C H C G + − + = • (2) In gas phase, Kº= (a b) (g h) b P A B h H g G K P P P P P P P P P + − + = •
(3)InheterogeneousphasesCO2(g) + H,O +Ca2+ = CaCO, (s) + 2H(aq)[H+]CoH+K=PcoCa2+]* Po [ca* ]1poCo
(3) In heterogeneous phases CO2 (g) + H2O +Ca2+ = CaCO3 (s) + 2H+ (aq) Kº= + + + + = 2 2 2 2 2 2 Ca P P H C Ca P P C H CO CO
Example 1:At the temperature of 1000K,put 1.00mol SO,and1.00mol O,in a closed container of 5.00dm3,when equilibium isreached,0.85molSO,isformed.(1) Calculate K°,K, and K,of the reaction 2SO, + O, = 2SOat the temperature of1000K:( 2 ) Use thermodynamic data to calculate Kat thetemperatureof298K.Solution: (1) 2SO, (g) +O, (g) = 2SO, (g)01.00t=0 (mol)1.000.851.00-0.851.00—0.85/2eq= 0.15=0.575
Example 1: At the temperature of 1000K, put 1.00mol SO2 and 1.00mol O2 in a closed container of 5.00dm3 ，when equilibium is reached , 0.85mol SO3 is formed. （1）Calculate Kº,Kp and Kc of the reaction 2SO2 + O2 = 2SO3 at the temperature of 1000K; （ 2 ） Use thermodynamic data to calculate Kºat the temperature of 298K. Solution：(1) 2SO2 (g) + O2 (g) = 2SO3 (g) t=0 (mol) 1.00 1.00 0 t eq 1.00－0.85 1.00－0.85/2 0.85 = 0.15 = 0.575