Q66 E Use the PhET Reactions & Rat... [FREE SOLUTION]

Chapter 12: Q66 E (page 710)

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?

Short Answer

Expert verified

When the total energy line is below the transition state of the potential line, the reaction does not occur. Above the transition potential energy line, the reaction proceeds in the forward direction.

Step by step solution

Energy of Activation

For any single step chemical reaction, the peak of the transition state energy represents the Energy of Activation, E_afor the given reaction. For the forward reaction to occur, the reactants must have total energy \({\bf{E}}\left( {\bf{T}} \right) \ge {{\bf{E}}_{\bf{a}}}\).

Total energy less than transition state energy

Initially, when the total energy line is below the transition state potential energy the reactants have total energy less than the activation energy, and the reaction \({\bf{A + BC}} \to {\bf{AB + C}}\) does not occur.

Total energy greater than transition state energy

Above the transition potential energy line, the reactants have energy greater than the activation energy, so the reaction proceeds in the forward direction.