Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Related questions
Question
11. Use the data in Table 2 to make an Arrhenius plot. From the plot, determine the activation energy (in kJ) and the frequency factor (A) for the following reaction: ??4(?) + ?3(?) → ????????.
Table 2: Kinetic data for a reaction between methane and ozone
Temperature (K) k (?/?∙?)
260 2.26 x 10-5
265 3.65 x 10-5
270 6.76 x 10-5
275 1.14 x 10-4
280 1.87 x 10-4
285 3.03 x 10-4
290 4.83 x 10-4
295 7.58 x 10-4
300 1.171 x 10-3
305 1.783 x 10-3
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 2 steps with 1 images
Knowledge Booster
Similar questions
- Given that the reaction 2 H2(g) + O2(g)-> 2 H₂O(g) is exothermic, which of the following is true of the reaction 2 H₂O(g) 2 H2(g) + O2(g)? Its activation energy is lower than that of 2 H2(g) + O2(g) -> 2 H₂O(g) Its activation energy is the same as that of 2 H2(g) + O2(g) -> 2 H₂O(g). Its activation energy is higher than that of 2 H2(g) + O2(g) ->2 H₂O(g)- O There is no relationship between its activation energy and that of 2 H2(g) + O2(g)-> 2 H₂O(g).arrow_forwardNonearrow_forward5. 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.arrow_forward
- = O KINETICS AND EQUILIBRIUM Using the Arrhenius equation to calculate Ea from k versus T data The rate constant k for a certain reaction is measured at two different temperatures: k 81.0 °C 4.0×10¹¹ 137.0 °C 1.6x10¹2 temperature Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. Round your answer to 2 significant digits. E = 0 mol x10 X 1/5arrow_forwardThe activation energy of an uncatalyzed reaction is 86 kJ/mol. The addition of a catalyst lowers the activation energy to 61 kJ/mol Part A Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 24 °C? Express the ratio to two significant digits. ke/ku = 2.2 • 1o Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining Part B Assuming that the collision factor remains the same, by what factor will the catalyst increase the rate of the reaction at 128 °C? Express the ratio to two significant digits. ? ke/k, = 2.9 • 10² Submit Previous Answers Request Answer X Incorrect; Try Again; 8 attempts remainingarrow_forward3. You have a reaction that is run at 273°C and has a rate constant of 2.52 x 10/s. The same reaction is run at 157 °C and has a rate constant of 1.0 x 10-/s. What is the activation energy for this reaction? (R = 8.314 J/mol K) %3D 0.00898mols 102 sec 4. w for ate= k[NO2]?. The rate constant for this reaction: If yo tion for 5 minutes urd be the concentraarrow_forward
- The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy E= 54.0 kJ/mol. If the rate constant of this reaction is 2.0 × 10³ M¹s -1.-1 at 222.0 °C, what will the rate constant be at 272.0 °C? Round your answer to 2 significant digits. k = M .S Ś 囧arrow_forwardLabel the reaction profiles below as exothermic or endothermic and use them to calculate the activation energy of the forward and reverse reactions and the value of AH for the reaction. This is a reaction of profile of an 250 exothermic/endothermic reaction 200 PE 150 (kJ) Eaf = ...... 100 Ea, = 50 AH = Reaction pathway 100 This is a reaction of profile of an 80 exothermic/endothermic reaction 60 PE (kJ) A+B 40 Ear = C+D 20 Ear = ΔΗ Progress of the reactionarrow_forwardThe rate constant k for a certain reaction is measured at two different temperatures: temperature k 314.0 °C 2.1 x 10¹1 384.0 °C 4.3 × 10¹1 Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy E for this reaction. a Round your answer to 2 significant digits. kJ E = x10 a mol X Ś ?arrow_forward
- Determine the activation energy, Ea, (in kJ/mol) of the decomposition reaction, CH3CHO → CH4 + CO. k (M-1/2 s-1) T (°C) 0.01028 940 0.0655 1380arrow_forwardStep 1: (slow) Step 2: C0 (fast) = CI The particle models shown above represent a proposed two-step mechanism for the destruction of ozone (03) in the upper atmosphere. Based on the models, which of the following represents a species that acts as a catalyst for the reaction? 88.8arrow_forward4arrow_forward
arrow_back_ios
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning 
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY