The equilibrium constant (KP) is 0.13 at a particular temperature for the reacti

Question

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

Explanation / Answer

Kp = [NO2]^2/[N2O4] 0.13[N2O4] = [NO2]^2 From PV=nRT P (Pressure) is directly proportional to n (moles). As the volume is constant we can use the pressure as equivalent to moles. So for the first one substitute the pNO2 into the equilibrium equation and solve for pN2O4 [N2O4] = 0.137^2/0.15 = 0.118. As you have 0.144 which is too much the reaction will move back to the NO2 or to the right. 2.[N2O4] = 0.081^2/0.13 = 0.05 at equalibrium 3. [N2O4] = 0.132^2/0.13 shift to left 4. [N2O4] = 0.082^2/0.13 shift to right 5.[N2O4] = 0.064^2/0.13 shift ot right

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