Question

1. A 0.050-mol sample of NO2 was placed in a 10.0-L container and heated to 750 K. 2NO2(g) → 2NO(g) + O2(g) The total pressure of the equilibrium mixture as a result of the decomposition was 0.414 bar. What is the value of K at this temperature? 2. The equilibrium constant (Kw) for the equation H20(1) - H+(aq) + OH-(aq) was measured at several temperatures. Determine ArH (298K) for the reaction using the following data: T('C) 10 20 30 40 K 2.87E-15 6.45E-15 1.38E-14 2.80E-14 Plots should be done using a graphing program like Excel: hand in plots with the assignment

Answer 1

o o oso mol moles of No intially = PV = пят امراء L. bar.k ma R =0.08314 px 10 = 0,05 x0.08314 x450 p= 0.312 bar 2N (9) = 2 NOC + °(5) initial 0.312 Change -2P +2P tp equilibrium 0.312-21 2P p - Al equilibrium Total pressure a 0,414 bar 0.312-28 + 2 + p = 0.414 P = 0.414-0.312 (p=00102 bat kp = (PNo)" (P2) (PNoz)? kp = (2p)2(6) (0.312-2p) ? I Kp = 0.3639 bar