# 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. c. How much time is required for all the 1.25 x 10-2 M C2H5OH to decompose?

###### FREE Expert Solution

Given: plot of [A] versus time → therefore the reaction is a zeroth-order reaction

The integrated rate law for this reaction is:

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

y             mx         b

slope of the graph (m) = -k

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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.

c. How much time is required for all the 1.25 x 10-2 M C2H5OH to decompose?