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The following data are for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g) - CH4(g) + H2(g) + CO(g) [ CH3OCH3 ], M 6.51×102 3.26x10-2 22.7 1.63×10-2 8.15x103 time, min 45.4 68.1 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is | min. (2) Based on these data, the rate constant for this | order reaction is | min .

The following data are for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g) - CH4(g) + H2(g) + CO(g) [ CH3OCH3 ], M 6.51×102 3.26x10-2 22.7 1.63×10-2 8.15x103 time, min 45.4 68.1 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is | min. (2) Based on these data, the rate constant for this | order reaction is | min .

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter13: Chemical Kinetics
Section: Chapter Questions
Problem 13.16QE
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The following data are for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g) → CH4(g) + H2(g) + CO(g) 3.26x10-2 22.7 [ CH3OCH3 ], M 6.51×10-2 1.63×10-2 8.15x103 time, min 45.4 68.1 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is | min . (2) Based on these data, the rate constant for this order reaction is min -1.
Transcribed Image Text:The following data are for the gas phase decomposition of dimethyl ether at 500 °C. CH3OCH3(g) → CH4(g) + H2(g) + CO(g) 3.26x10-2 22.7 [ CH3OCH3 ], M 6.51×10-2 1.63×10-2 8.15x103 time, min 45.4 68.1 Hint: It is not necessary to graph these data. (1) The half life observed for this reaction is | min . (2) Based on these data, the rate constant for this order reaction is min -1.
Expert Solution
Step 1

The relationship between half-life and rate constant of the reaction (first-order reaction) is expressed as,

k=0.693t1/2......(1)

Where,

  • k is the rate constant.
  • t1/2 is the half-life of the reaction.
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