Phosgene, cocl2, gained notoriety as a chemical weapon in world war i. phosgene is produced by the reaction of carbon monoxide with chlorine, co(g) cl2(g) < > cocl2(g) the value of kc for this reaction is 5.79 at 570 k. what are the equilibrium partial pressures of the three gases if a reaction vessel initially contains a mixture of the reactants in which pco?

The question is incomplete, here is the complete question:

Phosgene, , gained notoriety as a chemical weapon in World War I. Phosgene is produced by the reaction of carbon monoxide with chlorine:  

The value of for this reaction is 5.79 at 570 K. What are the equilibrium partial pressures of the three gases if a reaction vessel initially contains a mixture of the reactants in which and ?

The equilibrium partial pressure of CO, is 0.257 atm, 0.257 atm and 0.008 atm respectively.

Explanation:

The relation of is given by:

= Equilibrium constant in terms of partial pressure

= Equilibrium constant in terms of concentration = 5.79

= Difference between gaseous moles on product side and reactant side =

R = Gas constant =

T = Temperature = 570 K

Putting values in above equation, we get:

We are given:

Initial partial pressure of CO = 0.265 atm

Initial partial pressure of chlorine gas = 0.265 atm

Initial partial pressure of phosgene = 0.00 atm

The given chemical equation follows:

Initial:            0.265      0.265

At eqllm:        0.265-x    0.265-x        x

The expression of for above equation follows:

Putting values in above equation, we get:

Neglecting the value of x = 8.59 because equilibrium partial pressure cannot be greater than initial pressure

So, the equilibrium partial pressure of CO =

The equilibrium partial pressure of

The equilibrium partial pressure of

Hence, the equilibrium partial pressure of CO, is 0.257 atm, 0.257 atm and 0.008 atm respectively.

43.452

step-by-step explanation:

284 times .153 = 43.452