The following reaction was studied at a given temperature: CH3CI(g) + H2O(g)→ CH3OH(g) + HCI(g) From the rate data below, determine the reaction orders. Exp [CH3CI], [H,O]o Initial Rate (M s1) 1 0.100 0.100 0.182 2 0.200 0.200 1.45 3 0.200 0.400 5.81 O CH3CI: first order H,O: first order O CH;CI: second order H2O: second order O CH3CI: second order H2O: first order O CH3CI: first order H,O: second order

The following reaction was studied at a given temperature: CH3CI(g) + H2O(g)→ CH3OH(g) + HCI(g) From the rate data below, determine the reaction orders. Exp [CH3CI], [H,O]o Initial Rate (M s1) 1 0.100 0.100 0.182 2 0.200 0.200 1.45 3 0.200 0.400 5.81 O CH3CI: first order H,O: first order O CH;CI: second order H2O: second order O CH3CI: second order H2O: first order O CH3CI: first order H,O: second 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

A chemistry graduate student is studying the rate of this reaction: 2HI (g) → H₂ (g) +1₂ (g) He fills a reaction vessel with HI and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 [HI] 0.0400M 0.0199M 0.20 0.0133 M 0.30 0.00994M 0.40 0.00795 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 X Ś
Using the data in the table, calculate the rate constant of this reaction. k= A+B → C + D Trial [A] (M) [B] (M) 1 0.290 0.380 2 0.290 1.03 3 0.464 0.380 Units Rate (M/s) 0.0163 0.119 0.0261
A chemistry graduate student is studying the rate of this reaction: 2SO3 (g) → 2SO₂(g) + O₂(g) He fills a reaction vessel with SO3 and measures its concentration as the reaction proceeds: time (minutes) 0 10. 20. 30. [so,] 0.0500M 0.0190M 0.0117 M 0.00847 M 40. 0.00663 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 ロ・ロ X
17. SHOW ALL YOUR WORK OGiven the following data, determine the order of the reaction with respect to NO(g). 2 NO(g) + Cl2(g)→ 2 NOCI(g) Experiment 1 [C2] (M) 0.0100 [NO] (M) Rate (M/s) 3.4 x 104 1.36 x 103 3.4 x 104 0.0300 0.0150 0.0150 0.0100 3 0.0400
I need help with both of the blank spaces with correct significant figures
A student studies the concentration of reactant A over time in a reaction and gathers the following data. Use a spreadsheet program (or graph on paper) to determine the order of the reaction with respect to [A] and the rate constant. Enter the numeric value of the rate constant with at least 2 sig figs. time (sec) 0 34.6 82.3 103.1 142.2 179.7 230.0 [A]t [M] 1.146 0.984 0.794 0.708 0.558 0.413 0.233
In a study to determine the rate of the following reaction: 2NO (g) + 0, (g) → 2NO, (g) the concentration of NO was 0.0450 Mat t = 5.0 s and 0.0225 Mat t= 650.0 s. What is the average rate of the reaction during this time period?
Consider the reaction I- + OCl- → OH-→ IO- + Cl- Determine the reaction's rate law using the given experimental data. Exp # [I-]o [OCl-]o [OH-]o Initial Rate (M/s) 1 0.0013 0.012 0.10 0.094 2 0.0026 0.012 0.10 0.187 3 0.0013 0.006 0.10 0.047 4 0.0013 0.012 0.20 0.047
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)
Consider the mechanism. O3 + NO, – NO, + O, NO, + NO, – N,O5 slow fast O, + 2 NO, – 0, + N,O5 Identify the rate law for the overall reaction based on the mechanism. rate = k[O,||NO,? rate = k[O3] rate = k[O3][NO,1 rate = k[NO,? k[NO, ][NO3] rate =
A chemistry graduate student is studying the rate of this reaction: 2C1,O, (g) 2Cl₂ (g) +50₂ (g) She fills a reaction vessel with C1₂05 and measures its concentration as the reaction proceeds: time (minutes) 0 10. 20. [C1,05] 40. 0.600M 0.172M 0.101 M 30. 0.0710M 0.0548M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 ロ・ロ X Ś
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.