initial rateConsider the following reaction and initial rate data:Experiment121342H₂(g) + 2NO (g) → 2H₂O (g) + N₂ (g)[NO] initial (M)0.136[H₂]initial (M)0.2120.2120.4240.8480.2720.5440.544Initial Rate (M/s)0.02480.09910.7931.58What is the overall order of the reaction?4th1stDOOOOOO2nd3rdOthWhat is the unit for the rate constant for this reaction?M-2 sMs-1M-25-1M² S-1M-15-1M-15-2M²s

Answered: Image /qna-images/answer/92d2b239-61ef-4c35-b817-af026ca00e02.jpg

initial rate Consider the following reaction and initial rate data: Experiment 1 2 3 4 2H₂(g) + 2NO (g) → 2H₂O (g) + N₂ (g) [H₂]initial (M) [NO] initial (M) Initial Rate (M/s) 0.212 0.136 0.0248 0.212 0.272 0.0991 0.424 0.544 0.793 0.848 0.544 1.58 What is the overall order of the reaction? 4th 1st 2nd 3rd Oth What is the unit for the rate constant for this reaction? M²s Ms 1 M-25-1 M² S-1 0 0 0 0 0 О M-15-1 M-152 M² s

initial rate Consider the following reaction and initial rate data: Experiment 1 2 3 4 2H₂(g) + 2NO (g) → 2H₂O (g) + N₂ (g) [H₂]initial (M) [NO] initial (M) Initial Rate (M/s) 0.212 0.136 0.0248 0.212 0.272 0.0991 0.424 0.544 0.793 0.848 0.544 1.58 What is the overall order of the reaction? 4th 1st 2nd 3rd Oth What is the unit for the rate constant for this reaction? M²s Ms 1 M-25-1 M² S-1 0 0 0 0 0 О M-15-1 M-152 M² s

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

The following initial rate data are for the reaction for the formation of phosgene from carbon monoxide and chlorine: со + Clz → COCI2 Initial Rate, Ms-1 Experiment [CO]o, M [CIz]o, M 2.45 0.399 1.43x10-28 2 2.45 0.798 |2.85х10-28 3 4.90 0.399 2.85x10-28 4 4.90 0.798 5.71x10-28 Complete the rate law for this reaction in the box below. Use the form k[A]m[B]^ , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n Rate = From these data, the rate constant is M-1s-1.
The decomposition of nitrosyl bromide is followed 2 NOBr → 2 NO + Br2 Time (s) [NOBr] (M) 0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00 0.0033 Determine the average rate over the entire experiment.
Consider the reaction A + 2B = C whose rate at 25 °C was measured using three different sets of initial concentrations as listed in the following table: [A] [B] (M) (M) 0.20 0.010 4.8x10-4 2 0.20 0.020 9.6x10-4 3 0.40 0.010 1.9x10-3 Trial 1 Rate (M/s) What is the rate law for this reaction? Express the rate law symbolically in terms of k, [A], and [B].
Consider the reaction: 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 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 Calculate the rate of [NO3] production at 0.84 M [NO2]and 1.4 M [03]. Final answer must be rounded off to 2 decimal places, and shall NOT have any units.
A chemistry graduate student is studying the rate of this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) She fills a reaction vessel with C1₂05 and measures its concentration as the reaction proceeds: time [C1,05] (seconds) 0 0.400M 10. 0.263 M 20. 0.173 M 30. 0.114M 40. 0.0751M Use this data to answer the following questions. Write the rate law for this reaction. x10 Calculate the value of the rate constant k. X Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 Ś ?
The kinetic data shown below were observed for the reaction: BF3 (g) + NH3 (g) ---------> F3B·NH3 (g) Trial # [BF3] (mol/L) [NH3] (mol/L) Rate (M/s) 1 0.250 0.250 0.2130 2 0.250 0.125 0.1065 3 0.200 0.100 0.0682 4 0.350 0.100 0.1193 5 0.175 0.100 0.0596 b. What is the order with respect to [BF3]? (Hint: provide the number for the order, i.e. fourth order = 4)
Reaction of nitrogen monoxide and hydrogen A student collects the data below for the reaction: 2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g) Trial [NO]i [H2]i Initial Rate (M/s) 1 0.050 M 0.050 M 0.0917 2 0.10 M 0.050 M 0.367 3 0.10 M 0.10 M 0.734 Write 2-3 sentences to describe how you determined the rate law for the reaction.
6
Do not give handwriting solution.
The data shows that the rate depends on the concentration of the reactants. How else can a chemist increase the rate of reaction?
The data below were collected for the following reaction: CH3CI (g) + 3 Cl2 (g) → CCI4 (g) + 3 HCI (g) [CH3CI](M) [Cl2](M) Initial Rate (M/s) 0.050 0.050 0.014 0.100 0.050 0.029 0.100 0.100 0.041 0.200 0.200 0.115 What is the order of the reaction with respect to CH3CI? What is the order of the reaction with respect to Cl2? Enter each of your answers numerically as integers or fractions (ex: 0, 1/2, 1, 3/2, 2, 3, etc). Write an expression for the reaction rate law.
Consider the balanced chemical equation. H₂O₂ (aq) +31 (aq) + 2H+(aq) → I3¯¯(aq) + 2H₂O(1) In the first 11.0 s of the reaction, the concentration of I drops from 1.000 M to 0.752 M. Part A Predict the rate of change in the concentration of H₂O2 (A[H₂O2]/At). Express the rate to three significant figures and include the appropriate units. A[H₂O₂]/At = Submit Request Answer Part B Value μÀ HÅ Δ[13]/Δt = Value Predict the rate of change in the concentration of I3 (A[13¯]/At). Express the rate to three significant figures and include the appropriate units. Submit Request Answer Units Units ? www. ?