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Chapter 12: Q32 E (page 705)
Describe how graphical methods can be used to determine the order of a reaction and its rate constant from a series of data that includes the concentration of A at varying times.
The method of graphical determination is described below.
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There are two molecules with the formula\({{\bf{C}}_{\bf{3}}}{{\bf{H}}_{\bf{6}}}\). Propene,\({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{CH = C}}{{\bf{H}}_{\bf{2}}}\), is the monomer of the polymer polypropylene, which is used for indoor-outdoor carpets. Cyclopropane is used as an anaesthetic:
When heated to 499\({\bf{^\circ C}}\), cyclopropane rearranges (isomerizes) and forms propene with a rate constant of\({\bf{5}}{\bf{.95 \times 1}}{{\bf{0}}^{{\bf{ - 4}}}}{{\bf{s}}^{{\bf{ - 1}}}}\). What is the half-life of this reaction? What fraction of the cyclopropane remains after 0.75 h at 499.5\({\bf{^\circ C}}\)?
Based on the diagrams in Exercise 12.82, which of the reactions has the fastest rate? Which has the slowest rate?
Atomic chlorine in the atmosphere reacts with ozone in the following pair of elementary reactions:
\({\bf{Cl + \;O3}}\left( {\bf{g}} \right){\bf{ - - - ClO}}\left( {\bf{g}} \right){\bf{ + \;O2}}\left( {\bf{g}} \right)\)(rate constant k1 )
\({\bf{ClO}}\left( {\bf{g}} \right){\bf{ + O - - - Cl}}\left( {\bf{g}} \right){\bf{ + \;O2}}\left( {\bf{g}} \right)\)(rate constant k2 )
Determine the overall reaction, write the rate law expression for each elementary reaction, identify any intermediates, and determine the overall rate law expression.
For the past 10 years, the unsaturated hydrocarbon 1,3-butadiene \(\left( {{\bf{C}}{{\bf{H}}_{\bf{2}}}{\bf{ = CH - CH = C}}{{\bf{H}}_{\bf{2}}}} \right)\) has ranked 38th among the top 50 industrial chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene:
The isomerization of cyclobutene to butadiene is first-order, and the rate constant has been measured as \({\bf{2}}{\bf{.0 \times 1}}{{\bf{0}}^{{\bf{ - 4}}}}{{\bf{s}}^{{\bf{ - 1}}}}\) at 150 \({\bf{^\circ C}}\) in a 0.53-L flask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 \({\bf{^\circ C}}\) with an initial pressure of 55 torr.
The first-order radioactive decay of iodine-131 exhibits a rate constant of 0.138 \({{\bf{d}}^{{\bf{ - 1}}}}\). What is the half-life for this decay?
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