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The equilibrium constant Kc for the decomposition of phosgene, COCl2, is 4.63 × 10−3 at 527°C:...

The equilibrium constant Kc for the decomposition of phosgene, COCl2, is 4.63 × 10−3 at 527°C: COCl2(g) ⇆ CO(g) + Cl2(g) Calculate the equilibrium partial pressure of all the components, starting with pure phosgene at 0.760 atm.

Solutions

Expert Solution

Kp = KC*(RT) deltan.

deltan= Change in number of moles during the reaction, CoCl2-<--->CO +Cl2

deltan=2-1= 1

R= 0.0821 L.atm/mole.K T=527+273=800K

Kp =4.63*10-3*(0.0821*800)1 =0.3

                                            CoCl2              CO              Cl2

Initial (atm)                            0.76               0                0

Change                                  -x                 x                x

equilibrium                         0.76-x             x                 x

x= partial pressure

KP= x2/(0.76-x)= 0.3

when solved using excel, x=0.351 atm

Hence at equilbrium Partial pressures : CoCl2= 0.76-0.351=0.409 atm

partial pressure of CO= partial pressure of Cl2= 0.351 atm

queen_honey_blossom answered 2 years ago
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