The equilibrium constant (KP) is 0.22 at a particular temperature for the reacti
ID: 967079 • Letter: T
Question
The equilibrium constant (KP) is 0.22 at a particular temperature for the reaction:
N2O4(g) 2NO2(g)
Given the following sets of initial conditions, what is the net change that must occur for the reaction to reach equilibrium? Does the reaction shift left to reach equilibrium, does the reaction shift right to reach equilibrium or is the reaction at equilibrium at these initial concentrations so no net change will occur?
equilibrium
left
right
PNO2 = 0.108 atm, PN2O4 = 0.146 atm
equilibrium
left
right
PNO2 = 0.075 atm, PN2O4 = 0.066 atm
equilibrium
left
right
PNO2 = 0.283 atm, PN2O4 = 0.14 atm
equilibrium
left
right
PNO2 = 0.122 atm, PN2O4 = 0.068 atm
equilibrium
left
right
PNO2 = 0.177 atm, PN2O4 = 0.142 atm
Explanation / Answer
Solution :-
Kp = 0.22
N2O4(g) < ----- > 2NO2(g)
Using the pressure values given in each case we can calculate the Qp and compare it Kp to determine the direction of the shift
1) PNO2 = 0.108 atm, PN2O4 = 0.146 atm
Qp= [NO2]^2/[N2O4]
= [0.108]^2/0.146
= 0.07989
Qp < Kp so it will shift to right side
2) PNO2 = 0.075 atm, PN2O4 = 0.066 atm
Qp= [NO2]^2/[N2O4]
= [0.075]^2/0.066
= 0.08523
Qp < Kp so it will shift to right side
3) PNO2 = 0.283 atm, PN2O4 = 0.14 atm
Qp= [NO2]^2/[N2O4]
= [0.283]^2/0.14
= 0.572
Qp > Kp so it will shift to left side
4) PNO2 = 0.122 atm, PN2O4 = 0.068 atm
Qp= [NO2]^2/[N2O4]
= [0.122]^2/0.068
= 0.22
Qp = Kp so it is at equilibrium
5) PNO2 = 0.177 atm, PN2O4 = 0.142 atm
Qp= [NO2]^2/[N2O4]
= [0.177^2/0.142
= 0.22
Qp = Kp so it is it at equilibrium
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