6. Dimethyl ether, CH3OCH3, decomposes at high temperatures as shown in the following equation: CH3OCH3(g) → CH4(g) + H₂(g) + CO(g) The following data were obtained when the partial pressure of CH3OCH3 was studied as this compound decomposed at 500 °C. Use these data to determine the order of this reaction. PCH30CH3 (mmHg) 312 Time (s) 0 (Answer: second order) 278 390 251 777 227 1195 157 3155

6. Dimethyl ether, CH3OCH3, decomposes at high temperatures as shown in the following equation: CH3OCH3(g) → CH4(g) + H₂(g) + CO(g) The following data were obtained when the partial pressure of CH3OCH3 was studied as this compound decomposed at 500 °C. Use these data to determine the order of this reaction. PCH30CH3 (mmHg) 312 Time (s) 0 (Answer: second order) 278 390 251 777 227 1195 157 3155

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

For the reaction 2 A + 4 B → 2 C + 4 D, what is the absolute magnitude of the rate of change for [B] when [C] is increasing at 4.5 M/s?
For the reaction 2 A + 4 B → 2 C + 4 D, what is the absolute magnitude of the rate of change for [B] when [C] is increasing at 2.0 M/s?
Two molecules of 1,3-butadiene (C4H6) form 1,5-cyclooctadiene, C8H12 at higher temperatures.2 C4H6(g) → C8H12(g) Use the following data to determine the order of the reaction the rate constant, k. (Note that the total pressure is the pressure of the unreacted C4H6 at any time and the pressure of the C8H12.) Time (min) Total Pressure (mmHg) 0 436 3.5 428 11.5 413 18.3 401 25.0 391 32.0 382 41.2 371
Using the above data, determine the order of the reaction with respect to A and B, and the rate law.
The rate constant for the decomposition of gaseous azomethane, CH3N=NCH3 → N2 + C₂H6 is 40.8 min¹ at 425 °C. Calculate the number of moles of CH3N=NCH3 and N₂ in a 1.00 L flask 0.0500 min after 2.00 g of CH3N=NCH3 is introduced.
Consider the following rate law for the reaction A + B → products. rate = k{A}2{B}2 The reaction is order with respect to A, order with respect to B, and order overall.
For the reaction 4 A + 5 B → 2 C + 3 D, what is the magnitude of the rate of change for [D] when [A] is decreasing at 0.730 M/s?
The decomposition of sulfuryl chloride (SO2Cl2) is a first-order process. The rate constant for the decomposition at 660 Kis 4.5×10−2s−1. A)If we begin with an initial SO2Cl2 pressure of 460 torr, what is the partial pressure of this substance after 63 s? B) At what time will the partial pressure of SO2Cl2 decline to one-third its initial value?
Consider the reaction 2AB(g) → A2(g) + B2(g). If [AB] at 96 minutes was 0.71OM and dropped to 0.520M by 320.minutes, calculate the rate of consumption during this time frame.
Given the same reactant concentrations, the reaction CO(g) + Cl2(g) → COCl2(g) at 249°C is 48.4 times as fast as the same reaction at 169°C. Calculate the activation energy for this reaction. Assume that the frequency factor is constant.
Consider the reaction 5Br−(aq)+BrO−3(aq)+6H+(aq)→3Br2(aq)+3H2O(l) The average rate of consumption of Br− is 1.26×10−4 M/s over the first two minutes. What is the average rate of formation of Br2 during the same time interval?
The decomposition of ethylene oxide (CH₂)2O(g) → CH4(g) + CO(g) is a first order reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 631 K.