(a)
Interpretation:
The equation for the overall reaction has to be given.
(b)
Interpretation:
The structural formulas for all the given species has to be given.
(c)
Interpretation:
From the given reaction, the rate determining step has to be identified.
(d)
Interpretation:
Whether the given reaction is endothermic or exothermic has to be checked.
Concept introduction:
Exothermic reaction:
If heat is released during a chemical or physical change those reactions are called as exothermic reactions.
Endothermic reaction:
If heat is absorbed during a chemical or physical change those reactions are called as endothermic reactions.
(e)
Interpretation:
The effect of temperature on the given reaction rate has to be explained.
Want to see the full answer?
Check out a sample textbook solutionChapter 12 Solutions
General Chemistry: Atoms First
- Acetone is one of the most important solvents in organic chemistry. It is used to dissolve everything from fats and waxes to airplane glue and nail polish. At high temperatures, it decomposes in a first-order process to methane and ketene (CH2═C═O). At 600°C, the rate constant is 8.7 × 10−3 s−1. (a) What is the half-life of the reaction? Give your answer in scientific notation. (b) How long does it take for 38% of a sample of acetone to decompose? (c) How long does it take for 81% of a sample of acetone to decompose? Give your answer in scientific notation.arrow_forward! (plz give proper explanation)arrow_forward(a) For a reaction A + B —> P, the rate is given by Rate = k[A]2 [B](i) How is the rate of reaction affected if the concentration of A is doubled?(ii) What is the overall order of reaction if B is present in large excess?(b) A first order reaction takes 23.1 minutes for 50% completion. Calculate the time required for 75% completion of this reaction.(Given: log 2 = 0.301, log 3 = 0.4771, log 4 = 0.6021)arrow_forward
- Sulfonation of benzene has the following mechanism:(a) Write an overall equation for the reaction.(b) Write the overall rate law for the initial rate of the reaction.arrow_forward1.) The anticancer drug cis-platin hydrolyzes in water with a rate constant of 1.5 ×10−3 min−1 at pH 7.0 and 25°C. Calculate the half-life for the hydrolysis reaction under these conditions. If a freshly prepared solution of cis-platin has a concentration of 0.053 M, what will be the concentration of cis-platin after 5 halflives? after 10 half-lives? 2.) Ethyl chloride decomposes to ethylene and HCl in a first-order reaction that has a rate constant of 1.6 × 10−6 s−1 at 650°C. What is the half-life for the reaction under these conditions? If a flask that originally contains 0.077 Methyl chloride is heated at 650°C, what is the concentration of ethyl chloride after 4 half-lives?arrow_forwardThe radioactive isotope 28Mg has a half-life of 20.9 hours. (a) What is the rate constant for this first-order reaction? (b) What fraction of the isotope remains after 24 hours? Assume 3 significant figures in your calculations.arrow_forward
- Dinitrogen pentoxide, N2O5, decomposes when heated in carbon tetrachloride solvent.N2O5 →2NO2 + 1/2 O2(g) If the rate constant for the decomposition of N2O5 is 6.2 x10-4/min, what is the half-life? (The rate law is first order in N2O5.)(a) How long would it take for the concentration of N2O5 to decrease to 25% of its initial value? (b) To 12.5% of its initial value?arrow_forwardExperiments show that each of the following redox reac-tions is second order overall:Reaction 1: NO₂(g)+CO(g) →NO(g)+CO₂(g) Reaction 2: NO(g)+O₃(g) →NO₂(g)+O₂(g) (a) When [NO₂] in reaction 1 is doubled, the rate quadruples.Write the rate law for this reaction.(b) When [NO] in reaction 2 is doubled, the rate doubles. Writethe rate law for this reaction.(c) In each reaction, the initial concentrations of the reactantsare equal. For each reaction, what is the ratio of the initial rateto the rate when the reaction is 50% complete?(d) In reaction 1, the initial [NO₂] is twice the initial [CO].What is the ratio of the initial rate to the rate at 50% completion?(e) In reaction 2, the initial [NO] is twice the initial [O₃]. Whatis the ratio of the initial rate to the rate at 50% completion?arrow_forwardThe enzyme urease catalyzes the reaction of urea, 1NH2CONH22, with water to produce carbon dioxide and ammonia. In water, without the enzyme, the reaction proceeds with a first-order rate constant of 4.15 * 10-5 s-1 at 100 °C. In the presence of the enzyme in water, the reaction proceeds with a rate constant of 3.4 * 104 s-1 at 21 °C. (a) Write out the balanced equation for the reaction catalyzed by urease.arrow_forward
- 6. The rate constant for the reaction, 2 N₂O5 (g) → 4 NO2 (g) + O2 (g), doubles when the temperature is raised from 295.65 K to 300.62 K. (a) Determine the activation energy (in kJ/mol) for the reaction, assuming that the pre- exponential factor, A, in the Arrhenius equation is independent of temperature. (b) At what temperature would you predict this rate constant to increase by another factor of 10 relative to its value at 300.62 K?arrow_forwardIdentify each of the following elementary reactions as unimolecular, bimolecular, or termolecular, and write the rate expression. Reaction Molecularity Rate expression (a) BrONO,BrO + NO, rate = (b) HO + NO, + ArHNO3 + Ar rate = (c) OH + HC-H20 + Cl rate = unimolecular bimolecular termoleculararrow_forwardThe following data was obtained from the reaction: (a) Determine the rate law. (b) Calculate the rate constant. (c) Calculate the initial rate, if [NO2~] = 0.1 M and [NH4+] = 0.1 Marrow_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