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Ch.14 - Chemical Kinetics

Tro 4th Edition

Ch.14 - Chemical Kinetics

Problem 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.

Verified step by step guidance

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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Related Practice

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.

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?

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)?

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?

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.

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?