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Pure phosgene gas (COCl2), 0.0340 mol, was placed in a 1.30-L container. t was heated t...

Pure phosgene gas (COCl2), 0.0340 mol, was placed in a 1.30-L container. t was heated t o730.0 K, and at equilibrium, the pressure of CO was found to be 0.513 atm. Calculate the equilibrium constant Kp for the reaaction:

CO(g) + Cl2(g) >< COCl2(g)

Solutions

Expert Solution

PV = nRT

P = 0.034 x0.0821 x730/ 1.3

   = 1.567atm (initial)

CO + Cl2 <-------------------> COCl2

1.567    1                                0                      initial

1.567 -x   1-x                          x                        equilibrium

but   at equilibirum

pCO = 1.567 -x= 0.513

         x = 1.054

pCOCl2 = x = 1.054

pCl2 = 1-x = 0.054

Kp =pCOCl2 /pCl2 xpCO

kp= 1.054/0.054x0.513

Kp    = 38.05 atm^-1

queen_honey_blossom answered 1 year ago
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