Concept explainers
A C−-D bond is harder to break than a C−-H bond, and, consequently, reactions in which C−-D bonds are broken proceed more slowly than reactions in which C−-H bonds are broken. What mechanistic information comes from the observation that perdeuterated benzene,
Trending nowThis is a popular solution!
Chapter 15 Solutions
EBK ORGANIC CHEMISTRY
Additional Science Textbook Solutions
Chemistry: A Molecular Approach (4th Edition)
General Chemistry: Atoms First
Organic Chemistry (9th Edition)
Essential Organic Chemistry (3rd Edition)
Organic Chemistry (8th Edition)
The Organic Chem Lab Survival Manual: A Student's Guide to Techniques
- Assuming that the mechanism for the hydrogenation of C2H4 given in Section 11-7 is correct, would you predict that the product of the reaction of C2H4. with D2 would be CH2DCH2D or CHD2CH3? How could the reaction of C2H4 with D2 be used to confirm the mechanism for the hydrogenation of C2H4 given in Section 11-7?arrow_forwardThe data below show the concentration of N2O5 versus time for the following reaction: N2O5 (g) → NO3 (g) + NO2(g) Time (s) [N2O5] (M) 1.000 25 0.822 50 0.677 75 0.557 100 0.458 125 0.377 150 0.310 175 0.255 200 0.210arrow_forwardThe first step in the heterogeneoushydrogenation of ethylene is adsorption of theethylene molecule on a metal surface. One proposed explanation for the “sticking” of ethylene to a metalsurface is the interaction of the electrons in the C—C π bond with vacant orbitals on the metal surface. (a) If thisnotion is correct, would ethane be expected to adsorb to a metal surface, and, if so, how strongly would ethane bindcompared to ethylene? (b) Based on its Lewis structure,would you expect ammonia to adsorb to a metal surfaceusing a similar explanation as for ethylene?arrow_forward
- The degradation of the antibiotic clindamycin stored at 343 K in aqueous solution at pH 4 is found to be first order with a rate constant of 2.49 x 10−7 s −1. Over the temperature range 320 K to 360 K theactivation energy was found to be 123.3 kJ mol−1. (a) Calculate the rate constant at 325 K.(b) The threshold for product safety is 1% degradation. At 295 K the time taken for 1% of the antibiotic to degrade is found to be close to 0.01/ k. Comment on the shelf-life of the drug.arrow_forwardA second-order-reaction of the type A +2 B→ P was carried out in a solution that was initially 0.075 mol dm3 in A and 0.030 mol dm3 in B. After 1.0 h the concentration of A had fallen to 0.045 mol dm3. (a) Calculate the rate constant. (b) What is the half-life of the reactants? The rate constant for the decomposition of a certain substance is 1.70 x 10-2 dm³ mol-¹ s¹ at 24°C and 2.01 x 10-2 dm³ mol-¹ s¹ at 37°C. Evaluate the Arrhenius parameters of the reaction. A reaction 2 AP has a third-order rate law with k = 3.50 x 104 dmº mol2 s¹. Calculate the time required for the concentration of A to change from 0.077 mol dm3 to 0.021 mol dm³.arrow_forwardA rate constant is found to fit the expression kr = Ae−(4972 K)/T with A = 4.98 × 1013 dm3 mol−1 s−1 near 25 °C. Calculate Δ‡G for the reaction at 25 °C; assume κ = 1.arrow_forward
- The formation of dinitrogen pentoxide is described by the following chemical equation: 2NO, (g) + O; (g) → 0, (g) + N,O5 (g) Suppose a two-step mechanism is proposed for this reaction, beginning with this elementary reaction: NO2 (g) + 03 (g) NO; (g) + 0, Suppose also that the second step of the mechanism should be bimolecular. Suggest a reasonable second step. That is, write the balanced chemical equation of a bimolecular elementary reaction that would complete the proposed mechanism.arrow_forwardSome reactions proceed through a chain mechanism involving radicals, which are highly reactive species with one or more unpaired electrons. The radicals are produced in initiation steps, through either thermal or photodissociation. Reactions in which the radical centre is transferred are called propagation steps. The radicals are lost in termination steps. Consider the following chain mechanism:(1) AH → A + H·(2) A → B· + C(3) AH + B· → A + D(4) A + B· → P(a) Identify the initiation, propagation, and termination steps.(b) Use the steady-state approximation to deduce that the decompositionof AH is f irst-order in AH.arrow_forwardAlcohol is removed from the bloodstream by a series of metabolic reactions. The first reaction produces acetaldehyde; then other products are formed. The following data have been determined for the rate at which alcohol is removed from the blood of an average male, although individual rates can vary by 25-30%. Women metabolize alcohol a little more slowly than men: [CH,OH] (M) 4.4 x 10-2 3.3 x 10-2 2.2 x 10-2 Rate (mol/L/h) 2.0 x 10-2 2.0 × 10-2 2.0 x 10-2 Determine the rate equation, the rate constant, and the overall order for this reaction.arrow_forward
- Conventional equilibrium considerations do not apply when a reaction is driven by light absorption and the steady-state concentration of products and reactants might differ significantly from equilibrium values. For instance, suppose the reaction A → B is driven by light absorption, and that its rate is Ia, but that the reverse reaction B → A is bimolecular and second order with a rate kr[B]2. What is the stationary state concentration of B? Why does this ‘photostationary state’ differ from the equilibrium state?arrow_forwardwrite a rate law for the following reaction if reaction order n=1 2 N2O5 (g) -> 4 NO2 (g) + O2 (g)arrow_forwardThe conversion of high molecular weight olefins into saturated hydrocarbons makes use ofH 2 and is a heterogeneous process catalyzed by nickel. Draw and describe the mechanismaccording to the LH mechanism.arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning