log [S208^2-] (mol/L) Log [1] mol/L a. Assuming the rate expression for this system is in the form, rate - k[I]*[S₂Os²], it should be possible to determine the values of x and y from the data obtained. Show why a plot of log(time) vs log[I] for runs 1-4 will give a slope of -x and log(time) vs. log[S2082] for runs 1, 5, 6, and 7 will give a slope of-y. b. Perform the graphing exercises listed above and determine the values of x and y. Insert your graphs from Excel here. Log (Time) vs Log [1] 0 -0.2 1/6 1.65 1.7 1.75 1.8 1.85 1.9 1.95 -0.4 -0.6 -0.8 -1 -1.2 -1.4 -1.6 -1.8 0 0 -0.5 y=-1.7303x+1.7465 R²=0.766 Log (Time) Log (time) vs. log [S208^2-] 0.5 y=-0.8502x - 0.0374 R² = 0.9882 -1 -1.5 -2 -2.5 log (Time) 1.5 2 2.5 -1.4 -1.52 -1.7 -2

log [S208^2-] (mol/L) Log [1] mol/L a. Assuming the rate expression for this system is in the form, rate - k[I]*[S₂Os²], it should be possible to determine the values of x and y from the data obtained. Show why a plot of log(time) vs log[I] for runs 1-4 will give a slope of -x and log(time) vs. log[S2082] for runs 1, 5, 6, and 7 will give a slope of-y. b. Perform the graphing exercises listed above and determine the values of x and y. Insert your graphs from Excel here. Log (Time) vs Log [1] 0 -0.2 1/6 1.65 1.7 1.75 1.8 1.85 1.9 1.95 -0.4 -0.6 -0.8 -1 -1.2 -1.4 -1.6 -1.8 0 0 -0.5 y=-1.7303x+1.7465 R²=0.766 Log (Time) Log (time) vs. log [S208^2-] 0.5 y=-0.8502x - 0.0374 R² = 0.9882 -1 -1.5 -2 -2.5 log (Time) 1.5 2 2.5 -1.4 -1.52 -1.7 -2

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 1ALQ: Define stability from both a kinetic and thermodynamic perspective. Give examples to show the...

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Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.
The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.
What is the difference between average rate, initial rate, and instantaneous rate?
The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
6. Phenyl acetate, an ester, reacts with water according to the equation The data in the table were collected for this reaction at 5°C. Time (s) [Phenyl acetate] (mol/L) 0 0.55 15.0 0.42 30.0 0.31 45.0 0.23 60.0 0.17 75.0 0.12 90.0 0.085 Plot the phenyl acetate concentration versus time, and describe the shape of the curve observed. Calculate the rate of change of the phenyl acetate concentration during the period 15.0 seconds to 30.0 seconds and also during the period 75.0 seconds to 90.0 seconds. Why is one value smaller than the other? What is the rate of change of the phenyl acetate concentration during the time period 60.0 seconds to 75.0 seconds? What is the instantaneous rate at 15.0 seconds?
Consider the zero-, first-, and second-order integrated rate laws. If you have concentration versus time data for some species in a reaction, what plots would you make to prove a reaction is either zero, first, or second order? How would the rate constant, k, be determined from such a plot? What does the y-intercept equal in each plot? When a rate law contains the concentration of two or more species, how can plots be used to determine k and the orders of the species in the rate law?
Phenyl acetate, an ester, reacts with water according to the equation The data in the table were collected for this reaction at 5 C. (a) Plot the phenyl acetate concentration versus time, and describe the shape of the curve observed. (b) Calculate the rate of change of the phenyl acetate concentration during the period 15.0 seconds to 30.0 seconds and also during the period 75.0 seconds to 90.0 seconds. Why is one value smaller than the other?
Experimental data are listed here for the reaction A 2 B. (a) Prepare a graph from these data; connect the points with a smooth line; and calculate the rate of change of [B] for each 10-second interval from 0.0 to 40.0 seconds. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. (b) How is the rate of change of [A] related to the rate of change of [B] in each time interval? Calculate the rate of change of [A] for the time interval from 10.0 to 20.0 seconds.
One possible mechanism for the decomposition of nitryl chloride, NO2CI, is What is the overall reaction? What rate law would be derived from this mechanism? What effect does increasing the concentration of the product NO2 have on the reaction rate?
The thermal decomposition of diacetylene, C4H2, was studied at 950 C. Use the following data (K. C. Hou and H. B. Palmer, Journal of Physical Chemistry. Vol. 60, p. 858, 1965) to determine the order of the reaction.
For the reaction A+BC, explain at least two ways in which the rate law could be zero order in chemical A.
For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.