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13 Dec 2019

Given the reaction of a cleavage in the gas phase described withthe equilibrium equation:


N2O4 (g) <-->2NO2 (g)


a) Write an expression for the equilibrium constant (Kp) whenusing the partial pressures PNO2 and

PN2O4 of the gas (in atm) scheduled for mass action law.


b) at a temperature equal to 50

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Elin Hessel
Elin HesselLv2
17 Dec 2019

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Related questions

The equilibrium constant (KP) is 0.21 at a particulartemperature for the reaction:

N2O4(g) <=> 2NO2(g)

Given the following sets of initial conditions, what is the netchange that must occur for the reaction to reach equilibrium? Doesthe reaction shift left to reach equilibrium, does the reactionshift right to reach equilibrium or is the reaction at equilibriumat these initial concentrations so no net change will occur?

Options: Equilibrium, Left, or Right

a. PNO2 = 0.225 atm,PN2O4 = 0.134 atm

b. PNO2 = 0.086 atm,PN2O4 = 0.064 atm

c. PNO2 = 0.130 atm,PN2O4 = 0.142 atm

d. PNO2 = 0.173 atm,PN2O4 = 0.142 atm

e. PNO2 = 0.151 atm,PN2O4 = 0.062 atm

for the reaction N2O4(g) <--> (equilibrium arrows) 2NO2(g),kp = 0.25 at a certain temperature. Calculate the equilibriumpressures of NO2(g) and N2SO4(g) if the initial pressures of thecomponents when placed in an otherwise empty container are asfollows initial PNO2 = 0.0 atm Initial PN2O4= 0.040 atm EquilibriumPNO2 = ? atm Equilibrium PN2O4 = ? atm How do I go about solvingthis?

The equilibrium constant (KP) is 0.13 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? 1.PNO2 = 0.137 atm, PN2O4 = 0.144 atm 2.PNO2 = 0.081 atm, PN2O4 = 0.05 atm 3.PNO2 = 0.132 atm, PN2O4 = 0.054 atm 4.PNO2 = 0.082 atm, PN2O4 = 0.13 atm 5.PNO2 = 0.064 atm, PN2O4 = 0.07 atm

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