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The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surface C2H5OH1g2 h C2H4 1g2
Chapter 12, Problem 12.63(choose chapter or problem)
The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surface C2H5OH1g2 h C2H4 1g2 1 H2O1g2 was studied at 600 K. Concentration versus time data were collected for this reaction, and a plot of [A] versus time resulted in a straight line with a slope of 24.00 3 1025 mol/L s. a. Determine the rate law, the integrated rate law, and the value of the rate constant for this reaction. b. If the initial concentration of C2H5OH was 1.25 3 1022 M, calculate the half-life for this reaction. c. How much time is required for all the 1.25 3 1022 M C2H5OH to decompose?
Questions & Answers
QUESTION:
The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surface C2H5OH1g2 h C2H4 1g2 1 H2O1g2 was studied at 600 K. Concentration versus time data were collected for this reaction, and a plot of [A] versus time resulted in a straight line with a slope of 24.00 3 1025 mol/L s. a. Determine the rate law, the integrated rate law, and the value of the rate constant for this reaction. b. If the initial concentration of C2H5OH was 1.25 3 1022 M, calculate the half-life for this reaction. c. How much time is required for all the 1.25 3 1022 M C2H5OH to decompose?
ANSWER:a. The rate law is: rate = k [C2H5OH]
The integrated rate law is: ln[C2H5OH] = -kt + ln[C2H5OH]_i