4. Variation of the rate constant with temperature for the first-order reaction 2N205(g) → 2N204(g) + 02(g) is given in the following table. Determine the activation energy for the reaction. T (K) k (s-) 298 1.74 X 10 6.61 x 10-5 2.51 x 10-4 308 318 328 7.59 x 10-4 338 2.40 X 10-3 Activation Energy Arrhenius Constant

4. Variation of the rate constant with temperature for the first-order reaction 2N205(g) → 2N204(g) + 02(g) is given in the following table. Determine the activation energy for the reaction. T (K) k (s-) 298 1.74 X 10 6.61 x 10-5 2.51 x 10-4 308 318 328 7.59 x 10-4 338 2.40 X 10-3 Activation Energy Arrhenius Constant

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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5. The reaction A →B+C is known to be first order in A. Below are data showing the concentration of A as a function of reaction time. Time, min [A], M 5.00 x 10-2 4.30 x 10-2 5 10 3.70 x 10-2 2.74 x 10-2 1.51 x 10-2 20 40 1.12 x 10-2 8.26 x 10-3 50 60 (a) What is the average rate of reaction between 5 and 20 min? Report the units as well as the numbers. (b) Plot the data above, showing the concentration of A as a function of the time. From your graph, determine the instantaneous rate of reaction at 40 min. Report the units as well as the numbers. (c) Plot In [A] versus time. Estimate the rate constant for this first-order reaction from your graph. Report the units as well as the numbers.
A certain first order reaction has k = 2.51 s-1 . If the initial concentration of the reactant is 6.50 M, how much will be left after two half lives (in M)? Give your answer to three sig figs
For the reaction A → products, concentration and time data were collected. Enter these data into the graphing tool to determine the reaction order. t Graphing Tool 0.0 25.0 50.0 73.0 [A] 3.40 2.28 1.53 1.02 In[A] 1.223775 0.824175 0.425268 0.019803 Clear All Data 1/[A] 0.294118 0.438596 0.653595 0.980392 [A] 3.4 2.822 2.244 1.666 1.088 0.51 [A] vs. t to 0 14.6 t (s) 0.0 25.0 50.0 75.0 In[A] vs. t 29.2 t 43.8 1/[A] vs. t 58.4 [A] (M) 3.40 2.28 1.53 1.02 73
The table shows the variation of the rate constant with temperature for the first-order reaction. 2N₂O5 (g) 2N₂O₂(g) + O₂(g) Determine graphically the activation energy for the reaction. Be sure your answer has the correct number of significant digits. T(K)|*(--) S 298. 1.74 x 10 308. 6.61 × 10 318. 2.52 × 10 328. 7.59 × 10 338. 2.40 × 10 - 5 -5 -4 -4 3 Note: Reference the Fundamental constants table for additional information.
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The rate of a certain reaction was studied at various T(K) k (s-1) temperatures. The table shows temperature (T) and rate 400 0.000108 constant (k) data collected during the experiments. Plot the 420 0.000626 data to answer the questions. 440 0.00310 What is the value of the activation energy, E, for 460 0.0134 this reaction? 480 0.0511 500 0.175 520 0.547 E, = kJ - mol- 1108.79 540 1.57 560 4.18 Incorrect 580 10.4 What is the value of the pre-exponential factor (sometimes called the frequency factor), A, for this reaction? A = 140 6.79 x10 Incorrect
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 table: Time (s) [A] (M) 0.00 0.600 1.50 0.325 3.00 0.178 4.50 0.095 6.00 0.050 7.50 0.028 9.00 0.015
what is the activation energy for a first-order reaction if k = 2.5 x 10-3 s-1 at 332 K and k = 0.15 s-1 at 375 K?
A certain 2nd order reaction is known to proceed by a two-step process such that k1<<k2. The forward reaction has an activation energy of 48 kJ/mole and the reverse reaction has an activation energy of 62 kJ/mole. Sketch the energy diagram for the reaction.
13. The following data give the temperature dependence of the rate constant for the reaction N₂O4 →→ 2NO21/202. Plot the data and calculate the activation energy of the reaction. T(K) 273 298 308 318 328 338 k (sec-¹) 7.87 x 10-7 3.46 x 10-5 1.35 x 104 4.98 x 104 1.50 x 10-³ 4.87 x 10-3