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Chapter 12: Q9E (page 702)

Go to the PhET Reactions & Rates interactive. Use the Single Collision tab to represent how the collision between monatomic oxygen (O) and carbon monoxide (CO) results in the breaking of one bond and the formation of another. Pull back on the red plunger to release the atom and observe the results. Then, click on 鈥淩eload Launcher鈥� and change to 鈥淎ngled shot鈥� to see the difference.

  1. What happens when the angle of the collision is changed?
  2. Explain how this is relevant to rate of reaction.

Short Answer

Expert verified
  1. When angle of collision is changed it affects the formation of bonds and breaking of bonds between monoatomic oxygen and carbon monoxide.
  2. Angle of collision increases or decreases the rate of reaction.

Step by step solution

01

Angle of collision

In order for a reaction to occur, the particles of the reactant must have enough energy, and must collide at the correct angle.

Collision between monoatomic oxygen and carbon monoxide results in breaking of one bond and the formation of another bond. When angle of the collision is changed the collisions between monoatomic oxygen and carbon monoxide effect in way that the collisions may be increase or decrease resulting in the formation and breaking of bonds. It depends on the angle of collision or proper orientation.

02

Relevant to the rate of reaction

Molecules of reactants must come into contact with each other before reaction. If the angle of collision is changed resulting in the collisions between monoatomic oxygen and carbon monoxide increase, the rate of reaction or formation and breaking of bonds increases.

If angle of collision is changed resulting in the collisions between monoatomic oxygen and carbon monoxide decrease, the rate of reaction or formation and breaking of bonds decreases.

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Most popular questions from this chapter

Use the PhET Reactions & Rates interactive simulation to simulate a system. On the 鈥淪ingle collision鈥� tab of the simulation applet, enable the 鈥淓nergy view鈥� by clicking the 鈥�+鈥� icon. Select the first A + BC鉄禔B + C reaction (A is yellow, B is purple, and C is navy blue). Using the 鈥渟traight shot鈥� default option, try launching the A atom with varying amounts of energy. What changes when the Total Energy line at launch is below the transition state of the Potential Energy line? Why? What happens when it is above the transition state? Why?

Use the PhET Reactions & Rates interactive simulation (http://openstaxcollege.org/l/ 16PHETreaction) to simulate a system. On the 鈥淪ingle collision鈥� tab of the simulation applet, enable the 鈥淓nergy view鈥� by clicking the 鈥�+鈥� icon. Select the first A + BC鉄禔B + C reaction (A is yellow, B is purple, and C is navy blue). Using the 鈥渁ngled shot鈥� option, try launching the A atom with varying angles, but with more Total energy than the transition state. Whathappenswhen the A atom hitstheBC molecule from different directions? Why?

Tripling the concentration of a reactant increases the rate of a reaction nine-fold. With this knowledge, answer the following questions:

  1. What is the order of the reaction with respect to that reactant?
  2. Increasing the concentration of a reactant by a factor of four increases the rate of a reaction four-fold. What is the order of the reaction with respect to that reactant?

Doubling the concentration of a reactant increases the rate of a reaction four times. With this knowledge, answer the following questions:

  1. What is the order of the reaction with respect to that reactant?
  2. Tripling the concentration of a different reactant increases the rate of a reaction three times. What is the order of the reaction with respect to that reactant?

Experiments were conducted to study the rate of the reaction represented by this equation.(2)\({\rm{2NO(g) + 2}}{{\rm{H}}_{\rm{2}}}{\rm{(g) }} \to {\rm{ }}{{\rm{N}}_{\rm{2}}}{\rm{(g) + 2}}{{\rm{H}}_{\rm{2}}}{\rm{O(g)}}\)Initial concentrations and rates of reaction are given here.

Experiment Initial Concentration

\(\left( {{\bf{NO}}} \right){\rm{ }}\left( {{\bf{mol}}/{\bf{L}}} \right)\)

Initial Concentration, \(\left( {{{\bf{H}}_{\bf{2}}}} \right){\rm{ }}\left( {{\bf{mol}}/{\bf{L}}} \right)\)Initial Rate of Formation of \({{\bf{N}}_{\bf{2}}}{\rm{ }}\left( {{\bf{mol}}/{\bf{L}}{\rm{ }}{\bf{min}}} \right)\)
1\({\bf{0}}.{\bf{0060}}\)\({\bf{0}}.{\bf{00}}1{\bf{0}}\)\({\bf{1}}.{\bf{8}} \times {\bf{1}}{{\bf{0}}^{ - {\bf{4}}}}\)
2\({\bf{0}}.{\bf{0060}}\)\({\bf{0}}.{\bf{00}}2{\bf{0}}\)\({\bf{3}}.{\bf{6}} \times {\bf{1}}{{\bf{0}}^{ - {\bf{4}}}}\)
3\({\bf{0}}.{\bf{00}}1{\bf{0}}\)\({\bf{0}}.{\bf{0060}}\)\({\bf{0}}.{\bf{30}} \times {\bf{1}}{{\bf{0}}^{ - {\bf{4}}}}\)
4\({\bf{0}}.{\bf{00}}2{\bf{0}}\)\({\bf{0}}.{\bf{0060}}\)\({\bf{1}}.{\bf{2}} \times {\bf{1}}{{\bf{0}}^{ - {\bf{4}}}}\)

Consider the following questions:(a) Determine the order for each of the reactants, \({\bf{NO}}\) and \({{\bf{H}}_{\bf{2}}}\), from the data given and show your reasoning.(b) Write the overall rate law for the reaction.(c) Calculate the value of the rate constant, k, for the reaction. Include units.(d) For experiment 2, calculate the concentration of \({\bf{NO}}\)remaining when exactly one-half of the original amount of \({{\bf{H}}_{\bf{2}}}\) had been consumed.(e) The following sequence of elementary steps is a proposed mechanism for the reaction.Step 1:Step 2:Step 3:Based on the data presented, which of these is the rate determining step? Show that the mechanism is consistent with the observed rate law for the reaction and the overall stoichiometry of the reaction.
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