IISSED THIS? Read Section 15.5. You can click on the Review nk to access the section in your e Text. he following data show the rate constant of a reaction measured several different temperatures. Temperature (K) Rate constant (1/s) 1.38x10-2 4.32x10-2 300 310 320 330 340 0.126 0.342 0.879 ▼ Part A Use an Arrhenius plot to determine the activation barrier (E₁) for the reaction. Express your answer using three significant figures. [ΨΕΙ ΑΣΦ Submit Request Answer Part B ? A = Use an Arrhenius plot to determine the frequency factor (A) for the reaction. Express your answer using two significant figures. [5] ΑΣΦ kJ/mol ?

IISSED THIS? Read Section 15.5. You can click on the Review nk to access the section in your e Text. he following data show the rate constant of a reaction measured several different temperatures. Temperature (K) Rate constant (1/s) 1.38x10-2 4.32x10-2 300 310 320 330 340 0.126 0.342 0.879 ▼ Part A Use an Arrhenius plot to determine the activation barrier (E₁) for the reaction. Express your answer using three significant figures. [ΨΕΙ ΑΣΦ Submit Request Answer Part B ? A = Use an Arrhenius plot to determine the frequency factor (A) for the reaction. Express your answer using two significant figures. [5] ΑΣΦ kJ/mol ?

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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use/make a graph since there is 5 data points
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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
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Initial rate data at a certain temperature is given in the table for the following reaction. [NOCI], (M) Initial rate of formation of Cl, (M/s) 2 NOCI(g) → 2 NO(g) + Cl, (g) 0.600 1.30 x 10-5 0.750 2.03 x 10-5 0.900 2.92 x 10-5 Determine the value and units of the rate constant, k. Units: k :
Consider the following reaction. Calculate the rate of reaction for trial 4.. 2 A + B →→ 2 C Trial [A]0 [B]0 [C]0 Rate (M/s) 1 0.28 0.43 0.053 7.668 2 0.56 0.43 0.053 15.336 3 0.28 0.86 0.053 30.672 4 0.77 0.45 0.053 ?
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Ⓒ Macmillan Learning Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool Add Row 10 total rows [A] [A] vs. t In[A] In[A] vs. t t (min) 0.0 2.0 4.0 6.0 1/[A] vs. t [A] (M) 1.00 0.66 0.43 0.28 1/[A] Clear All Data
14. Consider the initial rate data at a certain temperature for the reaction 2NO + 2H2l + 2H,O Experiment 但](M) NO] (M) Initial rate (M/s) 0.200 0.200 2.06x10-4 2. 0.200 0.400 8.24x10-4 3 0.400 0.400 1.65x10-3 a. Determine the rate law for the reaction. b. Calculate the rate constant.
General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning Initial-rate data at a certain temperature is given in the table for the reaction N,0,(g) NO(g) + NO,(g) [N,O,], (M) Initial rate (M/s) 0.100 0.480 0.200 0.9600 0.300 1.440 Determine the value and units of the rate constant. units: k =
Use the information provided in the table below to answer the next two questions. The reaction between reactants A and B was studied at-10 °C. The following results were obtained. Experiment Initial [A] (mol/L) Initial [B] (mol/L) Initial Reaction Rate (M/min) 1 0.10 0.10 0.18 0.10 0.20 0.36 3 0.20 0.20 1.45 11. What is the order with respect to [B]? (a) 1 (b) 2 (c) ½ (d) 0 12. What is the order with respect to [A]? (a) 1 (b) 2 (c) ½ (d) 0
The following initial rate data are for the reaction of ICl with hydrogen: 2 ICI + H Iz + 2 HCI Initial Rate, Ms! 1.57x10-2 3.13×10-2 6.24x10-2 0.125 Experiment [ICI]. M H), M 1 0.207 0.211 2 0.414 0.211 3 0.207 0.421 4 0.414 0.421 Complete the rate law for this reaction in the box below. Use the form k[A]"[B]" , where 'l' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = From these data, the rate constant is