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- For the reaction 2N2O5(g)4NO2(g)+O2(g) the following data were collected, where Rate=[N2O5]t Time (s) T = 338 K [N2O5] T=318K [N2O5] 0 1.00 101 M 1.00 101 M 100. 6.14 102 M 9.54 102 M 300 2.33 102 M 8.63 102 M 600. 5.41 1O3 M 7.43 102 M 900. 1.26 1O3 M 6.39 102 M Calculate Ea for tills reaction.First order: [A]o In———- = kt [A]t t1/2= .693/kConsider the reaction data. munew 1 A → products R T (K) 225 575 at least three significant figures in all values. What two points should be plotted to graphically determine the activation energy of this reaction? To avoid rounding errors, use x₁ = x2 = k (s¹) 0.392 0.635 % 5 Determine the rise run and slope of the line formed by these points At a E T G f6 40 6 23) Y H & 7 V v || BN U 18 J 8 M 19 9 y₁ = K y2 = L f1o ►II O O L 7 112 62°F 0 { [ C. insert 811 PM 9/28/2022 ] prt sc ← backspace pause dele
- A+B AB Trial [A] (M) [B] (M) Rate (M/s) 1. 0.200 0.200 2.00 x102 0.400 0.200 8.00x 10 3. 0.200 0.400 4.00 x 10 Vhat is the order for B in the reaction above? Edit Format Table e T?v a BIU A 12pt Paragraph v 2.3. The following reaction: A' (a) + B (ag + C (an)→ G* (ae) +2 H ) AH = -250 kJ There are two proposed mechanism: Mechanism 1 A' () + B aa) AB' a) + D (a) Step 1 AB" (a) (fast) + E (a) + Hm → G' sae) + H ) + D² (n) Step 2 (slow) Step 3 E (agi+ C (a) (fast) Mechanism 2: Step 1 AB' (a) A' (an) + B (ag) AB' (a) + C ja) (fast) Step 2 + G' (a) + 2 H() (slow) The reactions was determined to have the following rate law: r= k[A'][B] a) Which of the two proposed mechanisms is valid? Explain. b) List any reaction intermediates: catalysts: c) What is a rate determining step? d) If the activation energy for the overall forward reaction is 150 kJ, sketch the potential energy diagram for the above reaction; showing the overall reaction, the reaction mechanism, labelling the AHu, AHy, Eapu, Eag, reaction intermediates, and activated complex. rvs fwd drvs/which hre obes the hydrde ottarth CR)- CB cataly THE 25°C,3o min
- 1 The rate constant for the second-order reaction Z NO: (x)2 NO (2) +0 () s054 Msat 300C. (al How lon (in seconds) wouldttakke for the concentration of NO; to decrease from 0.62 Mto 0.28 M (bi Caleulate the hal iwethese twe cocentratonsalfa + O M 1.2 K/s & 53 | 2:16 PM docs.google.com/for What is the value of k for a first 5 order reaction whose half life %3D 2.37 minutes if [A]O= O.1 M * k=0.1 sec-1 k= 0.292 min-1 k=0.0211 min -1 k=0.0683 min-1 k= 0.0947 min-13A2B Reaction of the second order it = [A] 2 5 4 10 Compute t1/2 15 8 20 10 + 1/2, k t at concentration 7 / and
- on at diferent Inltlal concentrations of the reactants were determined experimentally and the following results were obtainec P 10 SAIP A +B→ products [A] [B] initial rate 0.010 0.025 1.90 x 10-5 0.020 0.025 7.60 x 10-5 0.020 0.050 3.04 x 10-4 What is the value of the rate constant? O 3.04 O 1.52 O 0.076 O 304 P 31°C acerFor an autocatalytic reaction : A → B + …… where -d[A]/dt = k[A][B]. Assume that [B]o ≠0 Letting [A] = Ao – x and [B] = Bo +x -d[A]/dt = -d[Ao -x]/dt = dx/dt and dx/dt = k[Ao- x] [Bo + x] Show that [B] = {[A]o + [B]o } / [Ao/Bo] exp{- [A]o + [B]0 }kt + 111:28 PM Sat Feb 4 What is the rate for the zero order reaction A→ Products when [A] = 0.200 M? (k = 3.57 M/min) Tap here or pull up for additional resources N ! @ # $ Question 20 of 34 % A & +