Consider the reaction:NO2 + 03 → NO3 + 02[NO,], M[02], MRate, M/s6.30 x 10-3Experiment0.210.700.630.651.89 x 10-230.210.353.15 x 10-340.420.356.30 x 10-3What is the rate order of NO2?Oth1st2nd3rdNone of the above

The question involves the concepts of chemical kinetics. we have been given reaction. we have to…

NO2 + 03 → NO3 + 02 [NO,], M [03], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 x 10-2 3.15 x 10-3 2 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 What is the rate order of NO2? Oth 1st 2nd Зrd None of the above

NO2 + 03 → NO3 + 02 [NO,], M [03], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 x 10-2 3.15 x 10-3 2 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 What is the rate order of NO2? Oth 1st 2nd Зrd None of the above

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Do not give handwriting solution.
Using the data in the table, calculate the rate constant of this reaction. k= A+B C+D Trial 1 2 3 Units [A] (M) 0.260 0.260 0.364 [B] (M) 0.350 0.945 0.350 Rate (M/s) 0.0167 0.122 0.0234
REACTION A +B + C Products [B](M) 1.0 2.0 1.0 1.0 Rate(M/s) 1.0E-4 4.0E-4 2.0E-4 2.0E-4 Trial 1 [A](M) [C](M) 1.0 0.010 1.0 0.010 3 1.0 0.020 2.0 0.010 Using the data in the table and the rate law below, identify the reaction order with respect to each reatant. Rate = k[A]M[B]^[c]P (Rate = k times [A] to the mth power times [B] to the nth power times [C] to the pth power) %3D
The data given below refers to the reaction: A(aq) + 2B(aq) --> D(aq) + C (ag) What rate law is consistent with this kinetic data? Trial [A], M [B], M Rate of formation of D, M/s 0.100 0.100 3.00 x 10 - 4 0.300 0.300 9.00 x 10 - 4 3 0.100 0.300 3.00 x 10 - 4 4 0.200 0.400 6.00 x 10 - 4 A Rate = k B Rate = k[A] Rate = k[B] Rate = k[A][B] O A O B O C O D
For the given data, what is the correct unit for the rate constant, k? Run [B] [C] Initial Rate (M/sec) 1 1.5 2.0 0.20 2 1.5 4.0 0.40 3 3.0 2.0 0.80
A reaction proceeds according to the following equation: 3 A+ 4B 2 C + D What is the rate of formation of D, if the magnitude of the rate of consumption of A is 0.530 Ms-¹? Please give your answer to 3 decimal places. + esc I F1 486 F2 80 F3 Question 1 of 5 000 000 F4 24 F5 2 C 8 DII DD n 4 7 +/- 1
O https://app.101edu.co A * Question 7 of 20 Determine the rate law for the reaction A+ B - C + D given the following experiment data. Initial Trial [A]o [B]o Rate A) Rate = k[A] %3D (M/min) B) Rate = k[A]? 1 0.25 0.40 7.25 C) Rate = k[A][B] %3D 2 0.75 0.40 21.5 D) Rate = k[A]°[B] %3D 3 0.50 0.80 14.5 E) Rate = k[A][B] 4 0.75 0.80 21.5 Delete F12 wwwn D F11 FI0 FO FB FS FO Backspace Num Lock F2 %3D 1 8. 6. 4 12 3 Wome E R Enter J K F S. Shift Poyblip Ctr Alt Home All
Use the previous example for the chemical reaction 2 HgCl₂(aq) + C₂O4²-(aq)→ 2 Cl(aq) + 2 CO₂ (g) + Hg₂Cl₂ (s) The following initial rates of reactions were determined for the reactant concentrations given: Experiment #[HgCl₂] 0.100 0.100 0.050 1 2 3 [C₂O4²-] 0.20 0.40 1.2 x 10-4 0.40 6.2 x 10-5 Initial rate (M/sec) 3.1 x 10-5 (a) Find the order of the reaction with respect to HgCl2₂. (b)Find the order of the reaction with respect to C₂04² (c)Write the rate law for this reaction. (d)Calculate the value for the rate constant based on the data for experiment #1 and provide the proper units.
A rate is equal to 0.0200 M/s. If A = 0.100 M and rate = kA]|B]2, what is the new rate if the concentration of A] is increased to 0.200 M? %3D %3D 0.0200 M/s 0.0400 M/s 0.0600 M/s 0.0800 M/s O 0.100 M/s
1 ok S t nces Experiment [H₂] [NO] 0.010 0.025 Be sure to answer all parts. The following data were collected for the reaction between hydrogen and nitric oxide at 700°C: 2H₂(g) + 2NO(g) > 2H₂O(g) + N₂(g) 1 2 3 Initial rate (M/s) 2.4 x 10-6 1.2 × 10-6 0.010 0.0125 0.6 x 10-6 0.0050 0.025 5 attempts left (b) Calculate the rate constant. Check my work (a) Determine the order of the reaction. Enter a number in the field below. Number: Units:
Determine the average rate of change of B from t = 0 s to t = 282 s. A2B rateB = M/s Time (s) 0 141 282 Concentration of A (M) 0.610 0.380 0.150
The following data was plotted for the Kinetics of Phenolphthalein lab. Based on the plots below, what is the rate law for the reaction with respect to phenolphthalein (PN)? 0.5 0.45 04 0.35 0.3 0.25 0.2 0.15 0.1 0.05 25 20 15 10 S 0 0 . . 20 20 . 40 40 Abs vs Time 60 80 1/Abs vs Time 60 80 ● 100 100 O Rate Rate = 0.0198 120 120 Rate = 0.8332 [PN]² Rate = 0.8332 [PN] O Rate = 0.8332 O Rate = 0.0198 [PN]² O Rate = 0.0198 [PN] 140 1400 0 -0.5 -1 -15 -2 -2.5 -3 3.5 0 20 40 In(Abs) vs Time 60 80 100 120 140 y = -0.0198x -0.8332