The rearrangement of cyclopropane to propene at 500 °C(CH2)3 CH3 CH=CH₂is first order in(CH2)3 with a rate constant of6.70 × 107 -4 5-¹.SIf the initial concentration of(CH2)3 is 0.0297 M, the concentration of(CH₂)3 will beM after 2955 s have passed.

Answered: Image /qna-images/answer/6fce20c2-ff9c-496c-a1d2-7b60f8b5abd8.jpg

The rearrangement of cyclopropane to propene at 500 °C (CH2)3 CH3 CH=CH₂ is first order in (CH2)3 with a rate constant of 6.70 x 10-4 s If the initial concentration of (CH2)3 is 0.0297 M, the concentration of (CH₂)3 will be M after 2955 s have passed.

The rearrangement of cyclopropane to propene at 500 °C (CH2)3 CH3 CH=CH₂ is first order in (CH2)3 with a rate constant of 6.70 x 10-4 s If the initial concentration of (CH2)3 is 0.0297 M, the concentration of (CH₂)3 will be M after 2955 s have passed.

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

The rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH,NCO(aq)–→(NH),CO(aq) is second order in NH,NCO. In one experinment, when the initial concentration of NH,NCO was 0.851 M, the concentration of NH NCO dropped to 0.177 M after 291 minutes had passed. Based on these data, the rate constant for the reaction is M'min!
The overall order of the following reaction 2A + 3B → 2C with the rate law expression: Rate = k[X]1[Y]2 is
Consider the following reaction: 2 CH3l (aq) C2H6 (g) + 12 (g) This reaction is first-order, and its rate constant, k at 25°C is 0.0115 s¹. a) If the initial concentration of CH3l is 6.75 M, what is the concentration of CH3I after the reaction has been carried out for 1.83 hours? Report your answer using most of the decimal places reported on your calculator. Do not use scientific notation [CH31]= M b) If the rate constant is increased by a factor of 2.36 when the temperature is raised from 25°C to 76.6 °C, what is the activation energy (in kJ/mol) for this reaction? Report your answer using most of the decimal places reported on your calculator. Do not use scientific notation Ea kJ/mol
The gas phase decomposition of dinitrogen pentoxide at 335 K N,O5(g)- →2 NO,(g) + ½ O2(g) is first order in N,Og with a rate constant of 4.70×10-3 s. If the initial concentration of N,0g is 0.175 M, the concentration of N,Og will be 2.15x102 M after have passed.
The rearrangement of ammonium cyanate to urea in aqueous solution at 50 NH,NCO(aq)–(NH,),CO(aq) is second order in NH,NC0 with a rate constant of 1.10×10 ² M1 min. If the initial concentration of NH,NCO is 0.904 M, the concentration of 4 NH,NCO will be M after 247 minutes have passed.
The gas phase decomposition of hydrogen peroxide at 400 °C H2O2(g)H20(g) + ½ O2(g) is second order in H2O2. In one experiment, when the initial concentration of H,O2 was 0.242 M, the concentration of H,O, dropped to 4.09×10 M after 23.5 seconds had passed. Based on these data, the rate constant for the reaction is M1s1.
The first-order rate constant for the decomposition of N₂O5, given below, at 70°C is 6.82 x 10-3 s-1. Suppose we start with 0.0500 mol of N₂O5 (g) in a volume of 4.5 L. 2 N₂O5(9)→ 4 NO₂(g) + O₂(g) (a) How many moles of N₂O5 will remain after 3.0 min? 0.0146 mol (b) How many minutes will it take for the quantity of N₂O5 to drop to 0.005 mol? min (c) What is the half-life of N₂O5 at 70°C? min
3. The decomposition of di-tert-butyl peroxide (DTBP) is a first order reaction with a half- life of 320. minutes at 135 °C and 100. min at 145 °C. Calculate the activation energy for this reaction. (C4H9)2O2(g) → 2 (CH3)2CO(g) + С₂H₁(g)
One of the reactions that occurs in polluted air in urban areas is 2NO2(g) + O3(g) –→N2O5(g) + O2(g). Assume that a species with the formula NO3 is involved in the mechanism, and the observed rate law for the overall reaction is rate = k[NO2][O3]. Propose a mechanism for this reaction that includes the species NO3 and is consistent with the observed rate law. NO2(g) + O3(g) – NO3(g) + O2(g) (fast) NO3(g) + NO2(g) → N2O5(g) (slow) NO2(g) + O3(g) – NO3(g) + O2(g) (fast) 4NO3(g) 2N2O5(g) + O2(g) (slow) NO2(g) + O3(g) –→ NO3(g) + O2(g) (slow) NO3(g) + NO2(g) → N2O5(g) (fast) NO2(3) + O3(g) → NO3(g) + O2(g) (slow) 4NO3(3) → 2N20O5(g) + O2(g) (fast)
The rearrangement of cyclopropane to propene at 500 °C (CH2)3 CH3CH=CH2 is first order in (CH2)3 with a rate constant of 6.70×10-4 s-1. If the initial concentration of (CH2)3 is 0.128 M, the concentration of (CH2)3 will be M after 2099 s have passed.
The decomposition of nitramide in aqueous solution at 25 °C NH₂ NO₂ (aq) → N₂O(g)+ H₂O(1) is first order in NH₂ NO2 with a rate constant of -1 4.70 × 10-5 S-¹ If the initial concentration of NH₂NO2 is 0.864 M, the concentration of NH₂ NO2 will be M after 32118 s have passed.
The decomposition of nitramide in aqueous solution at 25 °c NH2NO2(aq)N½O(g) + H20(1) is first order in NH2NO2. During one experiment it was found that when the initial concentration of NH2NO2 was 0.402 M, the concentration of NH2NO2 dropped to 7.40x10-2 M after 25187 s had passed. Based on this experiment, the rate constant for the reaction is s-1.