# Problem: The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surfaceC2H5OH (g) → C2H4 (g) + H2O (g)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 -4.00 x 10-5 mol/L•s. a. Determine the rate law, the integrated rate law, and the value of the rate constant for this reaction.

###### FREE Expert Solution

Recall the integrated rate laws.

For a zeroth-order reaction is as follows:

$\overline{){\mathbf{\left[}\mathbf{A}\mathbf{\right]}}_{{\mathbf{t}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{kt}}{\mathbf{+}}{{\mathbf{\left[}}{\mathbf{A}}{\mathbf{\right]}}}_{{\mathbf{0}}}}$
y               mx         b

Graph: [A] vs. t

For a first-order reaction is as follows:

y                 mx               b

Graph: ln [A] vs. t

For a second-order reaction is as follows:

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###### Problem Details

The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surface

C2H5OH (g) → C2H4 (g) + H2O (g)

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 -4.00 x 10-5 mol/L•s.

a. Determine the rate law, the integrated rate law, and the value of the rate constant for this reaction.