After mixing equal amounts of the two molecules, the solution achieved equilibrium at 25 ∘ C . 25 ∘C. The concentration at equil
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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.
The third option. The angular quantum number (
) can be any integer between 0 and 
. Therefore, for the third option, can be 0, 1, 2, 3, or 4—but not 5.