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Chapter 12: Q51 E (page 708)

Chemical reactions occur when reactants collide. What are two factors that may prevent a collision from producing a chemical reaction?

Short Answer

Expert verified

Collision theory is a theory that is used to predict the rates of chemical reactions, particularly those involving gases. The collision theory holds that for a reaction to take place, the reacting species (atoms or molecules) must come into contact with one another.

Collision theory is founded on the following premises:

The reacting species must collide in such a way that contact between the atoms that will become bonded together in the product is possible.

The collision must have enough energy to allow mutual penetration of the valence of the reacting species. Shells, allowing electrons to rearrange and form new bonds (and new chemical species).

Step by step solution

01

Reaction of carbon monoxide with oxygen

Carbon monoxide is a pollutant that is produced during the combustion of hydrocarbon fuels. Automobiles have catalytic converters that use a catalyst to carry out this reaction to reduce this pollutant. It is also a byproduct of gunpowder combustion that causes muzzle flash in many firearms. At high temperatures and pressure, the reaction is spontaneous if sufficient amounts of carbon monoxide and oxygen are present.

The collision of two molecules is the first step in the gas-phase reaction of carbon monoxide and oxygen:

\({\bf{CO}}\left( {\bf{g}} \right){\bf{ + }}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right) \to {\bf{C}}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right){\bf{ + O}}\left( {\bf{g}} \right)\)

In the primary case, the oxygen aspect of the carbon monoxide molecule collides with the oxygen molecule.

02

Formation of carbon dioxide

In the second case, the carbon aspect of the carbon monoxide molecule collides with the oxygen molecule. The second case truly favors the formation of carbon dioxide (O = C = O), which has a crucial carbon atom bonded to 2 oxygen atoms. This is an easy example of ways critical collision orientation is in generating the favored response product. Two possible collisions between carbon monoxide and oxygen molecules. The orientation of the colliding molecules influences whether or not a reaction between the two molecules occurs.

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Most popular questions from this chapter

Use the provided initial rate data to derive the rate law for the reaction whose equation is: \({\bf{OC}}{{\bf{l}}^ - }\)(aq) + \({{\bf{I}}^ - }\)(aq) 鉄禣I鈭�(aq) +\({\bf{C}}{{\bf{l}}^ - }\)(aq)

Trial

(\({\bf{OC}}{{\bf{l}}^ - }\)) (mol/L)

(\({{\bf{I}}^ - }\)) (mol/L)

Initial Rate (mol/L/s)

1.

0.0040

0.0020

0.00184

2.

0.0020

0.0040

0.00092

3.

0.0020

0.0020

0.00046

Determine the rate law expression and the value of the rate constant k with appropriate units for this reaction.

The reaction of \({\bf{CO}}\) with \({\bf{C}}{{\bf{l}}_{\bf{2}}}\) gives phosgene \(\left( {{\bf{COC}}{{\bf{l}}_{\bf{2}}}} \right)\), a nerve gas that was used in World War I. Use the mechanism shown here to complete the following exercises:(fast, \({{\bf{k}}_{\bf{1}}}\) represents the forward rate constant, \({k_{ - {\bf{1}}}}\)the reverse rate constant)\({\bf{CO}}\left( g \right){\rm{ }} + {\rm{ }}{\bf{Cl}}\left( g \right) \to {\bf{COCl}}\left( g \right)\)(slow, \({k_{\bf{2}}}\) the rate constant)\({\bf{COCl}}\left( g \right){\rm{ }} + {\rm{ }}{\bf{Cl}}\left( g \right) \to {\bf{COC}}{{\bf{l}}_{\bf{2}}}\left( g \right)\)(fast,\({k_{\bf{3}}}\)the rate constant)(a) Write the overall reaction.(b) Identify all intermediates.(c) Write the rate law for each elementary reaction.(d) Write the overall rate law expression.

Radioactive phosphorus is used in the study of biochemical reaction mechanisms because phosphorus atoms are components of many biochemical molecules. The location of the phosphorus (and the location of the molecule it is bound in) can be detected from the electrons (beta particles) it produces:

\(\begin{aligned}{l}_{{\bf{15}}}^{{\bf{32}}}{\bf{P}} \to _{{\bf{16}}}^{{\bf{32}}}{\bf{S + }}{{\bf{e}}^{\bf{ - }}}\\{\bf{rate = 4}}{\bf{.85 \times 1}}{{\bf{0}}^{{\bf{ - 2}}}}\,{\bf{da}}{{\bf{y}}^{{\bf{ - 1}}}}{{\bf{(}}^{{\bf{32}}}}{\bf{p)}}\end{aligned}\)

What is the instantaneous rate of production of electrons in a sample with a phosphorus concentration of \({\bf{0}}{\bf{.0033 M}}\)?

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.

In terms of collision theory, to which of the following is the rate of a chemical reaction proportional?

(a) the change in free energy per second

(b) the change in temperature per second

(c) the number of collisions per second

(d) the number of product molecules
See all solutions

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