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Ch.14 - Chemical Kinetics
All textbooksTro 4th EditionCh.14 - Chemical KineticsProblem 5
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Chapter 14, Problem 5

The tabulated data show the concentration of N2O5 versus time for this reaction: N2O5(g) → NO3(g) + NO2(g). Time (s) [N2O5] (M): 0 - 1.000, 25 - 0.822, 50 - 0.677, 75 - 0.557, 100 - 0.458, 125 - 0.377, 150 - 0.310, 175 - 0.255, 200 - 0.210. Determine the order of the reaction and the value of the rate constant. Predict the concentration of N2O5 at 250 s.

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1
insert step 1: Determine the order of the reaction by analyzing the concentration data. Test for zero, first, and second order reactions by plotting [N2O5] vs. time, ln[N2O5] vs. time, and 1/[N2O5] vs. time, respectively. The plot that yields a straight line indicates the order of the reaction.
insert step 2: Once the order is determined, use the appropriate integrated rate law to calculate the rate constant (k). For a first-order reaction, use ln[N2O5] = -kt + ln[N2O5]_0. For a second-order reaction, use 1/[N2O5] = kt + 1/[N2O5]_0.
insert step 3: Calculate the slope of the straight line from the plot that determined the order of the reaction. This slope is equal to the rate constant (k) for the reaction.
insert step 4: Use the integrated rate law with the calculated rate constant to predict the concentration of N2O5 at 250 s. Substitute the time (t = 250 s) into the equation and solve for [N2O5].
insert step 5: Verify the calculated concentration by checking if it aligns with the trend observed in the data. This ensures the accuracy of the determined reaction order and rate constant.
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Textbook Question

Indicate the order of reaction consistent with each observation.

a. The half-life of the reaction gets shorter as the initial concentration is increased.

b. A plot of the natural log of the concentration of the reactant versus time yields a straight line.

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Textbook Question

A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C c. By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)? d. By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)? e. By what factor does the reaction rate change if [C] is doubled? f. By what factor does the reaction rate change if the concentrations of all three reactants are doubled?

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Textbook Question

A reaction in which A, B, and C react to form products is zero order in A, one-half order in B, and second order in C. c. By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)? d. By what factor does the reaction rate change if [B] is doubled? e. By what factor does the reaction rate change if [C] is doubled? f. By what factor does the reaction rate change if [C] is doubled (and the other reactant concentrations are held constant)?

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Open Question
Is the question about drawing a diagram that depicts the energy progression of an endothermic chemical reaction with an activation energy twice the value of the reaction's enthalpy change formulated correctly?
Open Question
A reaction has a rate constant of 0.000122 s⁻¹ at 27 °C and 0.228 s⁻¹ at 77 °C. a. Determine the activation barrier for the reaction.
Open Question
Cyclopropane (C3H6) reacts to form propene (C3H6) in the gas phase. The reaction is first order in cyclopropane and has a rate constant of 5.87 * 10^-4 s^-1 at 485 °C. If a 2.5-L reaction vessel initially contains 722 torr of cyclopropane at 485 °C, how long will it take for the partial pressure of cyclopropane to drop to below 1.00 * 10^2 torr?