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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
?
<u>Answer:</u> The equilibrium partial pressure of CO, is 0.257 atm, 0.257 atm and 0.008 atm respectively.
<u>Explanation:</u>
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:
<u>Initial:</u> 0.265 0.265
<u>At eqllm:</u> 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.