Given the following data, determine the rate law for the reaction 2 NO(g) + O₂(8) 2 NO₂(g) Experiment 1 2 3 [NO] (M) 0.0100 0.0200 0.0200 [0₂] (M) 0.0400 0.0400 0.0800 a) Calculate the overall order of the reaction Rate (M/s) 1.6 x 10-4 3.2 x 10-4 1.28x 10-3 b) Calculate the value of the rate constant (no decimals) and add the units AN

Given the following data, determine the rate law for the reaction 2 NO(g) + O₂(8) 2 NO₂(g) Experiment 1 2 3 [NO] (M) 0.0100 0.0200 0.0200 [0₂] (M) 0.0400 0.0400 0.0800 a) Calculate the overall order of the reaction Rate (M/s) 1.6 x 10-4 3.2 x 10-4 1.28x 10-3 b) Calculate the value of the rate constant (no decimals) and add the units AN

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

Determine the rate law for the following reaction using the experimental data given below. 2NO+ O2 →→→→→→→ 2NO2 Experiment 1 2 3 O rate=k[NO][0₂] O rate=k[NO]²[0₂] rate=k[NO]²[0₂]² rate=k[NO]²[0₂]³ O rate=k[NO]4[0₂]³ [NO] (M) 0.0503 0.0247 0.0503 [0₂] (M) 0.0202 0.0202 0.0609 Rate (M/s) 0.355 0.0888 1.07
The data in the table below were obtained for the reaction: 2A+ 2B → 3C Experiment Number [A] (M) [В] (M) Initial Rate (M/s) 1 0.186 0.451 2.26 0.930 0.451 11.3 0.186 1.35 20.34 The rate law for this reaction is rate = O A. k[A]2 O B. k[A]²[B]2 O. k[A][B] O D. K[A][B]? O E. k[A]²[B]
3 Use the following kinetic data to determine the order of the reaction and the value of the rate constant. 2NOBr (g) 2 NO (g) + Br2 (g) (8 Time(s) [NOBr] 0 10 20 30 40 0.040 0.030 0.024 0.021 0.018 [18
physical chemistry
consider the rate data at a certain temp for the reaction 2NO(g) + 2H2(g) --> N2(g) + 2H2O(g) determine the order of the reaction with respect to nitrogen monoxide
Using the data in the table, calculate the rate constant of Trial [A] (M) [B] (M) Rate (M/s) this reaction. 1 0.310 0.230 0.0240 A + B → C + D 2 0.310 0.506 0.116 > 3 0.527 0.230 0.0408 Units k =
Using the data in the table, calculate the rate constant of Trial [A] (M) [B] (M) Rate (M/s) this reaction. 1. 0.400 0.210 0.0120 A +B C+D 2 0.400 0.525 0.0750 3 0.480 0.210 0.0144 Units k =
Given the following data, determine the rate law for the reaction 2 NO(g) + O2g)22 NO2(g) Experiment [NO] (M) [O2] (M) Rate (M/s) 1 0.0300 0.0200 3.6 x 10-4 2 . 0.0600 0.0200 7.2 x 10-4 3 0.0600 0.0400 14.4 x 10-4 a) Determine the order of the reaction for each reactant, N, and 02. b) Write the rate law rate equation. ' ) ) Determine the value of the rate constant. (
The following reaction is observed to be second order with respect to NO and first order with respect to Br2. Br2 (g) + 2NO (g) --> 2NOBr (g)
The data in the table below were obtained for the reaction: 2A + 2B — зс Experiment Number [A] (M) [B] (M) Initial Rate (M/s) 1 0.775 0.321 0.082 2 1.51 0.321 0.082 3 0.775 0.963 0.738 The rate law for this reaction is rate = O A. k[A][B]² B. k[B]2 c. k[A][B] O D. K[A]2{B] O E. K[A]²[B]2
The data below were collected for the following reaction: CH3CI(g) + 3 Cl2(g) CCI4(g) + 3 HCI(g) [CH3CI] / mol L-1 Initial Rate / mol L-1 s-1 Trial [Cl2] / mol L-1 1 0.050 0.050 0.0142 2 0.100 0.050 0.0290 3 0.200 0.200 0.115 What is the order of the reaction with respect to Cl2?
Using the data in the table, calculate the rate constant of Trial [A] (M) [B] (M) Rate (M/s) this reaction. 1 0.330 0.240 0.0110 A + B → C+D 2 0.330 0.576 0.0634 3 0.495 0.240 0.0165 Units k =