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At a certain temperature, 1.0 mol of N2O4 is allowed to dissociate as…
Question
At a certain temperature, 1.0 mol of N2O4 is allowed to dissociate as N2O4(g) <=> 2NO2(g). At equilibrium it is found to be 50% dissociated while the total pressure of the system is held at 1.0 atm. Calculate Kp (in atm) for the reaction. Give the answer as a decimal rounded to four decimal places.
✓ Verified answer: 1.3333checked by our engine — not a guess
Step-by-step solution
For N2O4 <=> 2NO2 starting with 1 mol, at dissociation alpha the moles are (1-alpha) N2O4 and 2*alpha NO2, total = 1+alpha.
Mole fractions: NO2 = 2alpha/(1+alpha), N2O4 = (1-alpha)/(1+alpha).
Kp = (P_NO2)^2/P_N2O4 = [4 alpha^2/(1-alpha^2)] * P.
With alpha = 0.5, P = 1: Kp = 4(0.25)/(1-0.25) = 1/0.75 = 1.3333 atm.
Final answer1.3333
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