2 NO(g) + Br2 (g) → 2 NOB1(g) Initial Rate Experiment NO] (M) [Br2] (M) (mol/L's) 1 1.0 x 10-2 2.0 × 10-2 2.4 x 10-2 2 4.0 x 10-2 2.0 × 10-2 0.384 3 1.0 x 10-2 6.0 x 10-2 7.2 x 10-2 What is the order of the reaction with respect to [NO] and [Br2], and what is the overall order of the reaction? Order with respect to [NO] = Order with respect to [Br2] = Overall order

2 NO(g) + Br2 (g) → 2 NOB1(g) Initial Rate Experiment NO] (M) [Br2] (M) (mol/L's) 1 1.0 x 10-2 2.0 × 10-2 2.4 x 10-2 2 4.0 x 10-2 2.0 × 10-2 0.384 3 1.0 x 10-2 6.0 x 10-2 7.2 x 10-2 What is the order of the reaction with respect to [NO] and [Br2], and what is the overall order of the reaction? Order with respect to [NO] = Order with respect to [Br2] = Overall order

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

What is the correct unit for the rate constant? 1. Ms^-1 2. M^2s^-2 3. M^-1s^-1 4. M^-2s^-1
For the reaction 2 NO(g) + O 2 (g) → 2 NO2 (g) have the following data. Experiment 1 2 3: [NO], M 0.010: 0.020: 0.010 [O 2 ], M 0.010 :0.010: 0.020 The speed of consumption of 2.5 x 10-5 1.0 x 10-4 5.0 x 10-5 NO, Ms -1 a) write the rate equation for the reaction b) calculate the rate constant
What would the rate constant of the reaction be given the following set of experiments? .
Using the following rate law and the experimental values given in the question figures, calculate k: Rate = k[F2][ClO2] [F2] (M) [ClO2] (M) Initial Rate (M/s) Experiment 1 0.5 0.5 0.300 Experiment 2 0.8 0.8 0.768 Experiment 3 0.5 0.8 0.480
A+B AB Trial [A] (M) [B] (M) Rate (M/s) 1 0.200 0.200 2.00 x 102 0.400 0.200 8.00 x 102 0.200 0.400 4.00 x 102 What is the rate constant for the reaction above? 3.
What is the rate law of the reaction below: NO (g) + NO (g) -> N202 (g) fast N202(g) + O2(g)-> 2NO2 (g) slow rate = k [NOJ?[02] rate = k [NO]2[02]2 rate k [NO][02] O rate = k [NO][o²j²
Calculate the rate constant, k, for the given data. 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
#2 please
A+B → Products Run 1 2 3 [A]o [B] (M) (M) 1 1 2 1 2 1 Initial Rate (M/sec) 1 2 4 Rate = k [A]² [B]. What is k (don't forget the units) = [k]?
The reaction of nitrogen dioxide and carbon monoxide in the gas state to form carbon dioxide and nitric oxide is represented by the equation: NO2(g)+CO(g)--->CO2(g)+NO(g) The following data were collected for the above reaction Experiment No [CO2] (M) [CO] (M) Initial Rate (M/s) 1 5.0*10-4 1.6*10-2 1.7*10-7 2 5.0*10-4 3.2*10-2 1.7*10-7 3 1.5*10-3 3.2*10-2 1.5*10-6 Determine the order of the reaction with respect to each reactant.
4. The following data were obtained for the follwing chemical reaction: 2A+38->2C+D Trial # Initial (A) Initial [B] Initial Rate of Formation (mmol/L) (mmol/L) of D (mmol/L."s) 1 4.0 6.0 1.60 2 2.0 6.0 0.80 3 4.0 3.0 0.40 (a) Determine the rate law equation for this reaction. Show your reasoning. (T: 2) (b) Find the rate constant, k, with units. (T: 2)
Use the following data to calculate the reaction rate law and the rate law constant for the system. ??(?)+?2(?)→???2(?) Trial Run [NO] (mol/L) [H2] (mol/L) Initial Rate (mol/L∙s) 1 0.001 0.004 0.002 2 0.002 0.004 0.008 3 . 0.003 0.004 0.018 4 0.004 0.001 0.008 5 0.004 0.002 0.016 6 . 0.004 0.003 0.024 a) rate = k[NO][H2]2, where k = 7 L2/mol2∙s b) rate = k[NO]2[H2], where k = 5.0x105 L2/mol2∙s c) rate = k[NO][H2], where k = 5.0x105 L2/mol∙s d) rate = k[NO]2[H2]3, where k = 3.0x10-7 L/mol2∙s