Practice ProblemATTEMPT
Show that the following two-step mechanism is consistent with the experimentally determined rate law of rate
Want to see the full answer?
Check out a sample textbook solutionChapter 14 Solutions
Chemistry
- PRACTICE ANOTHER Identify the reaction intermediate or intermediates in the following multi-step mechanism. (Separate substances in a list with a comma.) Overall: 4 NO + 3 O2 + 2 H2O → 4 HNO3Step 1: 2 NO + O2 → 2 NO2Step 2: 4 NO2 + O2 + 2 H2O → 4 HNO3 ??????arrow_forwardGiven the following data: Experiment [A] [B] Initial rate (mol/(L·s)) 1 0.5 0.03 1.5 ´ 10-4 2 1.0 0.03 6.0 ´ 10-4 3 1.0 0.48 9.6 ´ 10-3 Determine the reaction order of A Determine the reaction order of B Determine the rate constant K Determine the rate of the reaction if [A] = 0.8M and [B] = 0.2Marrow_forwardThe initial rate of the reaction between AA and BB was measured. From the data given,a. determine the order of each reactant,b. determine the order of the reaction,c. write the rate law andd. calculate the rate constant, k. Experiment A B initial rate #1 0.20M 0.10M 3.50x10-3M/s #2 0.40M 0.10M 7.00x10-3M/s #3 0.40M 0.40M 7.00x10-3M/s if a reaction is second order in B and the concentration of B increased from 0.0850M to 0.2975M, what should happen to the rate?arrow_forward
- Part A Consider the reaction 2H3PO4→P2O5+3H2O2H3PO4→P2O5+3H2O Using the information in the following table, calculate the average rate of formation of P2O5P2O5 between 10.0 and 40.0 ss. Time (ss) 0 10.0 20.0 30.0 40.0 50.0 [P2O5][P2O5] (MM) 0 2.50×10−3 5.50×10−3 7.30×10−3 8.50×10−3 9.10×10−3arrow_forwardSelect the rate law that corresponds to the data shown for the following reaction: 2 A + 3 B → 2C Initial [A] 0.15 M 0.15 M 0.45 M Initial [B] 0.12 M 0.24 M 0.24 M Initial Rate 0.10 M/s 0.20 M/s 1.80 M/s (One of the options below is correct) a. rate = k[A]3[B] b. rate = k[A]3[B]2 c. rate = k[A]3 d. rate = k[A]2[B] e. rate = k[A]2[B]3arrow_forwardA reaction, A + B ---> C obeys the following rate law: Rate= k[B]2. What are the orders of the reaction with respect to A and B? and what is the overall reaction order? All three listed in that order A, B & overall Group of answer choices 1, 2 & 2 0, 2 & 0 0, 2 & 2 1, 2 & 3arrow_forward
- A reaction was experimentally determined to follow the rate law, Rate = k[A] 2 where k = 0.456 s -1M -1. Starting with [A] o = 0.500 M, how many seconds will it take for [A] t = 0.250 M? answer options 2.85 x 10 -2 s 1.14 x 10 -1 s 5.48x10 -1 s 1.52 s 4.39 sarrow_forwardFor the reaction 2 NO(g) + O 2 (g) → 2 NO2 (g) have the following data. Experiment 1 2 3: [NO], M 0.010: 0.020: 0.010 [O 2 ], M 0.010 :0.010: 0.020 The speed of consumption of 2.5 x 10-5 1.0 x 10-4 5.0 x 10-5 NO, Ms -1 a) write the rate equation for the reaction b) calculate the rate constantarrow_forwardSulfur dioxide reacts with carbon monoxide according to the following balanced reaction. The initial rate of reaction was measured in a series of experiments at 25 ∘C∘C as shown in the table below. SO2(g)+3 CO(g) → 2 CO2(g)+SCO(g) Experiment [SO2], M[SO2], M [CO], M[CO], M Initial reaction rate 1 0.0100 0.0100 0.0291 2 0.0250 0.0250 0.1150 3 0.0250 0.0100 0.0460 Part A Determine the overall order for the reaction. Enter your answer as a numerical value. Part B Calculate the value of the rate constant for the reaction. Express your answer with three significant figures. Do not include the unit. Part C What is the correct unit of the rate constant? Select one option. M−1.5⋅s−1M−1.5⋅s−1 M−2⋅s−0.5M−2⋅s−0.5 M−0.5⋅s−1M−0.5⋅s−1 M⋅s−1M⋅s−1 M−1⋅s−1M−1⋅s−1 None of the above are correct. Calculate the intial rate of appearance of carbon dioxide when 0.0500 MM SO2SO2 and 0.0675 MM COCO are…arrow_forward
- Sulfur dioxide reacts with carbon monoxide according to the following balanced reaction. The initial rate of reaction was measured in a series of experiments at 25 ∘C∘C as shown in the table below. SO2(g)+3 CO(g) → 2 CO2(g)+SCO(g) Experiment [SO2], M[SO2], M [CO], M[CO], M Initial reaction rate 1 0.0100 0.0100 0.0291 2 0.0250 0.0250 0.1150 3 0.0250 0.0100 0.0460 Part A Determine the overall order for the reaction. Calculate the value of the rate constant for the reaction. Express your answer with three significant figures. Do not include the unit. Calculate the intial rate of appearance of carbon dioxide when 0.0500 MM SO2SO2 and 0.0675 MM COCO are reacted. Express your answer with three significant figures and include the unit.arrow_forward. Consider the following reaction between mercury(II) chloride and oxalate ion: 2HgCl2(aq) + C2O42- ® 2Cl-(aq) + 2CO2(g) + Hg2Cl2(s) The initial rate of this reaction was determined for several concentrations of HgCl2 and C2O42-, and the following rate data were obtained: Experiment [HgCl2] (M) [C2O42-] (M) Rate (M/s) 1 0.105 0.15 1.8 x 10-5 2 0.105 0.30 7.1 x 10-5 3 0.052 0.30 3.5 x 10-5 4 0.052 0.15 8.9 x 10-6 a) What is the rate law for this reaction? b) What is the value of the rate constant? c) What is the reaction rate when the concentration of HgCl2 is 0.080 M and that of C2O42- is 0.10 M if the temperature is the same as in the above experiments?arrow_forwardPlease check! 1.Determine the overall reaction order for the reaction, A+B→2C using the table of data below: Experiment Initial [A]/M Initial [B]/M Initial rate/M s-1 1 0.010 0.040 0.0031 2 0.010 0.020 0.0015 3 0.020 0.020 0.0032 a. 0 b. 1 c. 2 <-- I think it's this one b/c the numbers are doubled in the table. d. 3 2. The overall order for the reaction, A+B→C, is 2. A student tests this by measuring the reaction rate at one concentration of A and B, then doubling both concentrations at the same time and re-measuring the rate, which quadrupled. The student concludes that the data support the hypothesis that the above rate law is rate=k[A][B]. Analyze this. a. The data do support the hypothesis but each trial should be repeated. b. The data contradict the hypothesis because the rate should have doubled, not quadrupled. <-- c. The data support the hypothesis but a trial holding one reactant constant is needed. b. The data contradict the hypothesis but testing by…arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples 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 EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY