Chemistry, 19.03.2020 22:42 Nyasiabaltimore3
He equilibrium constant (KP) is 0.21 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?
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
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He equilibrium constant (KP) is 0.21 at a particular temperature for the reaction:
N2O4...
N2O4...
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