v=k[acetic anhydride]a [water]b However, the reaction will take place in a dilute aqueous solution so that the concentration of water will hardly change. Thus we can write the rate law as follows v = keff [acetic anhydrideja We will determine this effective rate constant and the reaction order with respect to acetic anhydride in both light water (H₂O) and heavy water (D₂O). What method or approximation has been used here to transform the rate law? isolation method method of initial rates steady-state approximation rate-determining step approximation pre-equilibrium approximaiton

v=k[acetic anhydride]a [water]b However, the reaction will take place in a dilute aqueous solution so that the concentration of water will hardly change. Thus we can write the rate law as follows v = keff [acetic anhydrideja We will determine this effective rate constant and the reaction order with respect to acetic anhydride in both light water (H₂O) and heavy water (D₂O). What method or approximation has been used here to transform the rate law? isolation method method of initial rates steady-state approximation rate-determining step approximation pre-equilibrium approximaiton

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...

See similar textbooks

Similar questions

For the gas phase isomerization of cis-cyanostyrene, cis-C6H5CH=CHCN_trans-C%HşCH=CHCN the rate constant at 677 K is 5.01x10-4 51 and the rate constant at 717 K is 3.39x10-35-1. What is the activation energy for this reaction? kJ/mol
4. Write the free radical chain mechanism for the following bromination reaction: BrCC13 hv + Br HCC13
The activation energy for the gas phase decomposition of 2-bromopropane is 212 kJ.CH3CHBrCH3CH3CH=CH2 + HBrThe rate constant at 672 K is 3.16×10-4 /s. The rate constant will be 3.76×10-3 /s at K.
In the unimolecular gas phase reaction kinetics, what is the rate equation for the deactivation of the energized molecule A*? d[A*]/dt=-k'a[A] [A*] d[A*]/dt=ka[A]? O d[A*]/dt=-k½[A*] d[A*]/dt=k[A*]
The following initial rate data are for the reaction of tertiary butyl bromide with hydroxide ion at 55 °C: (CH3)3CB + OH → (CH3)3COH + Br Experiment [(CH3)3CB1],, M [OH], M Initial Rate, Ms-1 1 0.890 1.50x10-3 1.50x10-3 3.01x10-3 3.01x10-3 0.118 0.118 2 1.78 0.890 1.78 3 0.237 4 0.237 Complete the rate law for this reaction in the box below. Use the form k[A]j™[B]" , where '1' 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
4. Explain why the rate of formation of 1-azidopropane is different depending on which halopropane (X = F, Cl, Br, I) is used. Explain which halopropane will react fastest? ~X X = F, Cl, Br, I NaN №3 1-azidopropane
The activation energy for the gas phase decomposition of acetic anhydride is 144 k). (CH3CO)20→CH2=C=0 + CH3COOH The rate constant at 502 K is 9.94x10 4/s. The rate constant will be 9.74x10 3/s at K.
Alkoxides R-O can be used to synthesize alkenes as exemplified by the reaction shov below, where the symbol (et) indicates that the substance is dissolved in ethanol (CH,CH,OH) used as solvent: Br + (1) Br(et) (et) + (et) CH,CH,OH + t-but-Br Ethoxide Isobutylene 10. What is the value of the rate constant for the synthesis of isobutylene at 25 °C? а) 6.8 х10-8 Trial Initial Initial Initial Rate (M/s) [t-but-Br] [Ethoxide] [isobutylene] b) 8.5 x10-7 6.8 x 10-8 13.6 х 10-8 1 0.08 M 0.04 M c) 2.1 x 10-5 0.16 M 0.04 M 0.08 M 0.08 M 6.8 x 10-8 13.6 x 10-8 d) 1.1 x10-5 3 0.08 M 4 0.16 M