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Chapter 12: Q67 E (page 710)

Use the PhET Reactions & Rates interactive simulation (http://openstaxcollege.org/l/ 16PHETreaction) to simulate a system. On the “Single collision” tab of the simulation applet, enable the “Energy view” by clicking the “+” icon. Select the first A + BC⟶AB + C reaction (A is yellow, B is purple, and C is navy blue). Using the “angled shot” 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?

Short Answer

Expert verified

In both cases, the reaction rate depends on the orientation and energy of the reactants.

In all the cases where reactant A hits the molecule BC from different directions, the reaction rate depends on the orientation and energy of the reactants.

Step by step solution

01

A hits BC from different directions

When Reactant A hits BC from different directions, not all collisions lead to the forward reaction.

02

Explanation

Reactant A has sufficient energy to react with BC. However, proper orientation of the molecules is required to bring about the reaction. So proper orientation along with total energy will determine product formation.

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Most popular questions from this chapter

The reaction of compound A to give compounds C and D was found to be second-order in A. The rate constant for the reaction was determined to be 2.42 L/mol/s. If the initial concentration is 0.500 mol/L, what is the value of t1/2?

Use the PhET Reactions & Rates interactive simulation to simulate a system. On the “Single collision” tab of the simulation applet, enable the “Energy view” by clicking the “+” icon. Select the first A + BC⟶AB + C reaction (A is yellow, B is purple, and C is navy blue). Using the “straight shot” 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?

How will each of the following affect the rate of the reaction:

\({\bf{CO}}\left( {\bf{g}} \right){\bf{ + \;N}}{{\bf{O}}_{\bf{2}}}\left( {\bf{g}} \right) \to {{\bf{O}}_{\bf{2}}}{\bf{\;}}\left( {\bf{g}} \right){\bf{ + NO}}\left( {\bf{g}} \right)\) if the rate law for the reaction is rate = \({\bf{k(NO}}{}_{\bf{2}}{\bf{)(CO)}}\)?

  1. Increasing the pressure of \({\bf{NO}}{}_{\bf{2}}\) from 0.1 atm to 0.3 atm
  2. Increasing the concentration of CO from 0.02 M to 0.06 M.

The half-life of a reaction of compound A to give compounds D and E is 8.50 min when the initial concentration of A is 0.150 mol/L. How long will it take for the concentration to drop to 0.0300 mol/L if the reaction is (a) first order with respect to A or (b) second order with respect to A?

Regular flights of supersonic aircraft in the stratosphere are of concern because such aircraft produce nitric oxide, NO, as a by-product in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction \({\bf{NO + }}{{\bf{O}}_{\bf{3}}} \to {\bf{N}}{{\bf{O}}_{\bf{2}}}{\bf{ + }}{{\bf{O}}_{\bf{2}}}\) is first order with respect to both NO and \({{\bf{O}}_{\bf{3}}}\) with a rate constant of \({\bf{2}}{\bf{.20 \times 1}}{{\bf{0}}^{\bf{7}}}{\bf{mol}}{{\bf{L}}^{{\bf{ - 1}}}}{{\bf{s}}^{{\bf{ - 1}}}}\). What is the instantaneous rate of disappearance of NO when \(\left( {{\bf{NO}}} \right){\bf{ = 3}}{\bf{.3 \times 1}}{{\bf{0}}^{{\bf{ - 6}}}}{\bf{ M}}\) and \({\bf{(}}{{\bf{O}}_{\bf{3}}}{\bf{) = 5}}{\bf{.9 \times 1}}{{\bf{0}}^{{\bf{ - 7}}}}{\bf{ M}}\)?
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