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 K_p for the reaaction:

CO(g) + Cl₂(g) >< COCl₂(g)

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

p_CO = 1.567 -x= 0.513

x = 1.054

p_COCl2 = x = 1.054

p_Cl2 = 1-x = 0.054

Kp =p_COCl2 /p_Cl2 xp_CO

kp= 1.054/0.054x0.513

Kp = 38.05 atm^-1

queen_honey_blossom answered 7 months ago

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