The rate of a certain reaction was studied at various T(K) k (s-') temperatures. The table shows temperature (T) and rate 400 0.000278 constant (k) data collected during the experiments. Plot the data to answer the questions. 420 0.00189 440 0.0108 What is the value of the activation energy, E,, for 460 0.0532 this reaction? 480 0.229 500 0.878 520 3.03 E, = kJ - mol- 540 9.56 560 27.8 580 74.9 What is the value of the pre-exponential factor (sometimes called the frequency factor), A, for this reaction? A =

The rate of a certain reaction was studied at various T(K) k (s-') temperatures. The table shows temperature (T) and rate 400 0.000278 constant (k) data collected during the experiments. Plot the data to answer the questions. 420 0.00189 440 0.0108 What is the value of the activation energy, E,, for 460 0.0532 this reaction? 480 0.229 500 0.878 520 3.03 E, = kJ - mol- 540 9.56 560 27.8 580 74.9 What is the value of the pre-exponential factor (sometimes called the frequency factor), A, for this reaction? A =

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Consider the following reaction data. Reaction [A] (M) [B] (M) Rate (M/s) 1 0.100 0.100 10 0.200 0.100 40 3 0.100 0.200 20 The generic rate law equation is: rate = k[A]*[B]Y What is the value of x?
30. The following data were collected for a certain reaction of the type: A → products Time, min [A], mol L-1 0 0.300 1 0.284 2 0.268 3 0.252 0.236
use chart provided
For the reaction A products, concentration and time data were collected. t (s) [A] (M) > 0.0 3.40 Enter these data into the graphing tool to determine the reaction order. 25.0 2.28 50.0 1.53 75.0 1.02 Graphing Tool Clear All Data [A] vs. t In[A] vs. t 1/[A] vs. t t [A] In[A] 1/[A] [V]
D Time and concentration data were collected for the reaction A products t (s) -0 20 40 60 80 100 [A] (M) 0.52 0.43 0.35 0.29 0.23 0.19 The blue curve is the plot of the data. The straight orange line is tangent to the blue curve at t = 40 s. Approximate the instantaneous rate of this reaction at time t = 40 s. 25 instantaneous rate: M/s 0.52- 0.48 0.44 0.40 0.36- 0.32- 0.28- 0.24- 0.20- 0.16 0 10 20 30 40 50 60 70 80 90 t(s)
The tabulated data shows the concentration of N2O5 versus time for the reaction: N2O5=NO3+NO2 Time, s [N2O5], M 0 1.0 25 .822 50 .677 75 .557 100 .458 125 .377 150 .310 175 .255 200 .210 Determine the order of the reaction.
CHAPTER 12 Chemical Kinetics 81. The following data were obtained for the reaction 2A + B → C where rate = d{A]/dt [A](M) [B](M) Initial Rate(M/s) 0.100 0.0500 2.13 x 10-4 0.200 0.0500 4.26 x 10-4 0.300 0.100 2.56 x 10-3 Determine the value of the rate constant. a) 0.426 b) 0.852 c) 0.0426 d) 0.284 e) none of these
Consider the data below for the following reaction: A → Products - Reaction Time (s) [A](M) 0.000 0.541 28.16 0.329 61.75 0.223 88.92 0.178 Which best describes the order of this reaction?
Consider the table of data collected for the reaction A~ Products. Determine the magnitude (value) of the reaction rate constant by graphing the data appropriately.
The rate constant dependence on temperature of a chemical reaction is plotted below ( LnK versus 1/T). Calculate the Ea(Activation Energy) in kJ/mol (GIVEN: 8.314 J K-1 mol-1) * y= -4423x+3.665 -11.8 -11.85 -11.9 -11.95 -12 -12.05 -12.1 0.0035 0.00352 0.00354 0.00356 1/T (K') 83.14 kJ/mol 36.77 kJ/mol 44.33 kJ/mol 3.05 kJ/mol 36.60 kJ/mol In k
The rate of a certain reaction was studied at various temperatures. The table shows temperature (?) and rate constant (?) data collected during the experiments. Plot the data to answer the questions. What is the value of the activation energy, ?a , for this reaction? ? (?) ? (?−1) 400 0.000659 420 0.00327 440 0.0181 460 0.0589 480 0.213 500 0.615 520 1.66 540 3.99 560 9.64 580 20.1 Ea= What is the value of the pre‑exponential factor (sometimes called the frequency factor), ? , for this reaction?
3) The rate constant for the reaction 2 N20(g) → 2N2(g) + O2(g) has been found to vary with temperature according to the following data. Determine the activation energy for the reaction. (Must include best fit graph). e 1°C k /s1 565 728 757 780 1.10 x 10-3 0.380 0.871 1.67