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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

01

Energy of Activation

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

02

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.

03

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.

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Most popular questions from this chapter

Nitro-glycerine is an extremely sensitive explosive. In a series of carefully controlled experiments, samples of the explosive were heated to 160 掳C, and their first-order decomposition was studied. Determine the average rate constants for each experiment using the following data:

Initial (\({{\bf{C}}_{\bf{3}}}{{\bf{H}}_{\bf{5}}}{{\bf{N}}_{\bf{3}}}{{\bf{O}}_{\bf{9}}}\)) (M)

4.88

3.52

2.29

1.81

5.33

4.05

2.95

1.72

t(s)

300

300

300

300

180

180

180

180

% Decomposed

52.0

52.9

53.2

53.9

34.6

35.9

36.0

35.4

Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value of the rate constant, k, for the reaction was measured at several different temperatures, and the data are shown here:

Temperature(K)

k(M-1s-1)

555

6.23*10-7

575

2.42*10-6

645

1.44*10-4

700

2.01*10-3

What is the value of the activation energy (in kJ/mol) for this reaction?

For each of the following reaction diagrams, estimate the activation energy \(\left( {{E_a}} \right)\)of the reaction:

The rate constant for the rate of decomposition of \({{\bf{N}}_{\bf{2}}}{{\bf{O}}_{\bf{5}}}\)to\({\bf{NO}}\) and \({{\bf{O}}_{\bf{2}}}\)in the gas phase is 1.66 L/mol/s at 650 K and 7.39 L/mol/s at 700 K:

\({\bf{2}}{{\bf{N}}_{\bf{2}}}{{\bf{O}}_{\bf{5}}}{\bf{(g) - - - 4NO(g) + 3}}{{\bf{O}}_{\bf{2}}}{\bf{(g)}}\)

Assuming the kinetics of this reaction are consistent with the Arrhenius equation, calculate the activation energy for this decomposition.

In an experiment, a sample of NaClO3 was 90% decomposed in 48 min. Approximately how long would this decomposition have taken if the sample had been heated 20掳C higher?
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