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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 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?

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

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?

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?

The hydrolysis of the sugar sucrose to the sugars glucose and fructose, \({{\bf{C}}_{{\bf{12}}}}{{\bf{H}}_{{\bf{22}}}}{{\bf{O}}_{{\bf{11}}}}{\bf{ + }}{{\bf{H}}_{\bf{2}}}{\bf{O}} \to {{\bf{C}}_{\bf{6}}}{{\bf{H}}_{{\bf{12}}}}{{\bf{O}}_{\bf{6}}}{\bf{ + }}{{\bf{C}}_{\bf{6}}}{{\bf{H}}_{{\bf{12}}}}{{\bf{O}}_{\bf{6}}}\) follows a first-order rate equation for the disappearance of sucrose: \({\bf{Rate = k}}\left( {{{\bf{C}}_{{\bf{12}}}}{{\bf{H}}_{{\bf{22}}}}{{\bf{O}}_{{\bf{11}}}}} \right)\) (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.)

  1. In neutral solution, \({\bf{k = 2}}{\bf{.1 \times 1}}{{\bf{0}}^{{\bf{ - 11}}}}{{\bf{s}}^{{\bf{ - 1}}}}\) at 27 掳C and \({\bf{8}}{\bf{.5 \times 1}}{{\bf{0}}^{{\bf{ - 11}}}}{{\bf{s}}^{{\bf{ - 1}}}}\) at 37 掳C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 掳C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature).
  2. When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is\({\bf{1}}{\bf{.65 \times 1}}{{\bf{0}}^{{\bf{ - 7}}}}{\bf{ M}}\). How long will it take the solution to reach equilibrium at 27 掳C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible.
  3. Why does assuming that the reaction is irreversible simplify the calculation in part (b)?

Account for the relationship between the rate of a reaction and its activation energy.

Compare the functions of homogeneous and heterogeneous catalysts.
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