In a container, the partial pressure of NOCl is initially 0.340 atm at a given t
ID: 941579 • Letter: I
Question
In a container, the partial pressure of NOCl is initially 0.340 atm at a given temperature. The chemical equation which describes the reaction is:
At equilibrium analysis shows the partial pressure of NO is 0.0916 atm.
a) Which direction did the reaction proceed to establish (reach) equilibrium?
b) What is the partial pressure of NOCl which reacted in order for the partial pressure of NO to be 0.0916 atm?
c) What is the partial pressure of Cl2 at equilibrium?
d) What is the magnitude of KP for the equation above?
Explanation / Answer
a) Which direction did the reaction proceed to establish (reach) equilibrium?
NO initial = 0
NO equil = 0.0916;
there is a shift toward REACTANTS
b) What is the partial pressure of NOCl which reacted in order for the partial pressure of NO to be 0.0916 atm?
according to the extent
PNO = 0.0916
then
PNOCl = 0.34 - 0.0916 = 0.2484 atm
c) What is the partial pressure of Cl2 at equilibrium?
must be that half of NO, since ratio is 1:2
PCL2 = 0.0916 /2 = 0.0458
d) What is the magnitude of KP for the equation above?
Kp = (NOCl^2)/(NO^2)(Cl2)
Kp =0.2484 ^2 / ((0.0916 ^2)*0.0458) = 160.5634
Kp =160.5634