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Ch.14 - Chemical Kinetics
All textbooksTro 4th EditionCh.14 - Chemical KineticsProblem 51
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Chapter 14, Problem 51

The tabulated data show the concentration of cyclobutane (C4H8) versus time for this reaction: C4H8 -> 2 C2H4. Time (s) [C4H8] (M) 0 1.000 10 0.894 20 0.799 30 0.714 40 0.638 50 0.571 60 0.510 70 0.456 80 0.408 90 0.364 100 0.326. Determine the order of the reaction and the value of the rate constant. What is the rate of reaction when [C4H8] = 0.25 M?

Verified step by step guidance
1
<insert step 1> Start by plotting the concentration of cyclobutane, [C_4H_8], versus time to visually inspect the data and determine if it fits a zero, first, or second-order reaction.>
<insert step 2> For a zero-order reaction, a plot of [C_4H_8] versus time should be linear. For a first-order reaction, a plot of ln[C_4H_8] versus time should be linear. For a second-order reaction, a plot of 1/[C_4H_8] versus time should be linear.>
<insert step 3> Calculate the natural logarithm of the concentration, ln[C_4H_8], and the reciprocal of the concentration, 1/[C_4H_8], for each time point.>
<insert step 4> Plot ln[C_4H_8] versus time and 1/[C_4H_8] versus time to determine which plot is linear. The linear plot will indicate the order of the reaction: first-order if ln[C_4H_8] is linear, second-order if 1/[C_4H_8] is linear.>
<insert step 5> Once the order is determined, use the slope of the linear plot to calculate the rate constant, k. For a first-order reaction, the slope of ln[C_4H_8] versus time is -k. For a second-order reaction, the slope of 1/[C_4H_8] versus time is k. Then, use the rate law to calculate the rate of reaction when [C_4H_8] = 0.25 M.>
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Textbook Question

Indicate the order of reaction consistent with each observation. a. A plot of the concentration of the reactant versus time yields a straight line. Indicate the order of reaction consistent with each observation b. The reaction has a half-life that is independent of initial concentration. c. A plot of the inverse of the concentration versus time yields a straight line.

Textbook Question

Indicate the order of reaction consistent with each observation c. The half-life of the reaction gets longer as the initial concentration is increased.

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Textbook Question

The tabulated data show the concentration of AB versus time for this reaction: AB( g)¡A( g) + B( g) Time (s) [AB] (M) 0 0.950 50 0.459 100 0.302 150 0.225 200 0.180 250 0.149 300 0.128 350 0.112 400 0.0994 450 0.0894 500 0.0812 Determine the order of the reaction and the value of the rate constant. Predict the concentration of AB at 25 s.

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Textbook Question

The reaction A¡products was monitored as a function of time. The results are shown here. Time (s) [A] (M) 0 1.000 25 0.914 50 0.829 75 0.744 100 0.659 125 0.573 150 0.488 175 0.403 200 0.318 Determine the order of the reaction and the value of the rate constant. What is the rate of reaction when [A] = 0.10 M?

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Textbook Question

This reaction was monitored as a function of time: A → B + C A plot of ln[A] versus time yields a straight line with slope -0.0045/s. a. What is the value of the rate constant (k) for this reaction at this temperature?

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Textbook Question

This reaction was monitored as a function of time: A → B + C A plot of ln[A] versus time yields a straight line with slope -0.0045/s. b. Write the rate law for the reaction.