Find the value of the specific rate constant at 710 K. Express your answer using two significant figures. VE ΑΣΦ Submit Part B Request Answer [C2H5 Cl]-[C2H5 C1] t [C₂H5 C1]0 Find the fraction of the ethyl chloride that decomposes in 15 minutes at this temperature. Express your answer using one significant figure. V—| ΑΣΦ Submit Request Answer Part C ? T = 8-1 Find the temperature at which the rate of the reaction would be twice as fast. Express your answer using two significant figures. —| ΑΣΦΑ ? 2 ? K

Find the value of the specific rate constant at 710 K. Express your answer using two significant figures. VE ΑΣΦ Submit Part B Request Answer [C2H5 Cl]-[C2H5 C1] t [C₂H5 C1]0 Find the fraction of the ethyl chloride that decomposes in 15 minutes at this temperature. Express your answer using one significant figure. V—| ΑΣΦ Submit Request Answer Part C ? T = 8-1 Find the temperature at which the rate of the reaction would be twice as fast. Express your answer using two significant figures. —| ΑΣΦΑ ? 2 ? K

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...

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If a temperature increase from 10.0 ∘C∘C to 23.5 ∘C∘C doubles the rate constant for a reaction, what is the value of the activation barrier for the reaction? Express your answer using three significant figures.
[RCOOH], M [R’OH], M [HA], M Initial Rate, M-min 23. 0.35 0.35 0.50 4.60 0.62 0.35 0.50 8.14 0.35 0.81 0.50 10.6 0.35 0.50 0.75 9.84 Rate = k[RCOOH][R'OH] Rate = k[RCOOH][R'OH][HA] Rate = k[RCOOR']/{[RCOOH][R'OH]} Rate = k[R'OH] Rate = k[RCOOH] 26. The initial reaction rate for the reaction in question 23 can be followed spectrophotometrically by quenching the reaction and determining the amount of R'OH left by its reaction with the dichromate ion, Cr20-2-. Write a balanced equation for the reaction of Cr20,2- with R'OH in acid solution. For simplicity, you may assume R' is an ethyl group (CH3CH2) and the products of the reaction are Cr3+ and CH3COOH. ЗСНЗСН20Н() + 2Cr2072-(аq) + 16H+{аq) + 3СНЗСООН() 4C13+(aq) + 3CH3COOCH3(I) + 14H2O(1) --> 3CH3CH2OH(I) + 2Cr2072-(aq) + 16H+(aq) ЗСНЗСООН() + 11Н20() 4Cr3+(aq)+ + --> --> 4CR3+(aq)++ 3CH3CH2OH(I) + 2Cr2072-(aq) + 5H2O(I) ЗСНЗСООН() + 160H-(аq) CH3CH2OH(I) + Cr2072-(aq) 2Cr3+(aq)+ + CH3COOH(I) --> СНЗCН2ОH() + Cr2072-(aq) Cr3+(aq)+ +…
If the rate constant for the decomposition reaction of cyclobutane into ethylene is 2.08 x 10-2 s¹ at a certain temperature, how many seconds are required for the initial concentration (2.75) to decrease to 1.40? (Hint: What is the rate order based on k's units?) Your Answer: Answer units
When [F] is decreasing at 0.15mol/Lxs, how fast is [G] increasing? Be sure to use correct number of significant figures.
- 1 - 1 At a certain temperature this reaction follows second-order kinetics with a rate constant of 32.5M •S : NH,ОH (аq) -- Nн; (ад) +н,о (аq) Suppose a vessel contains NH,OH at a concentration of 0.910M. Calculate the concentration of NH,OH in the vessel 0.120 seconds later. You may assume '4 no other reaction is important. Round your answer to 2 significant digits. OM x10
Would this be the correct answer ?
I Review | Constants | Period MISSED THIS? Read Section 15.4 (Pages 642 - 649); Watch KCV 15.4, IWVE 15.4.The decomposition of SO2 Cl2 is first order in SO2 Cl2 and has a rate constant of 1.40x104s-1 at a certain temperature. -kt + In(SO2C2]o - (1.40 x 10-s)(220 s) + In 0.175 M In[SO2 Cl2]t %3D -1.774 Take the inverse natural logarithm of both sides of the equation. [SO2 Cl2]: e-1.774 M 0.170 M Part E If the initial concentration of SO2 Cl2 is 0.175 M, what is the concentration of SO2 Cl2 after 510 s ? Express your answer using three significant figures. ΑΣφ (SO2 Cl2]e = M
In a study of the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NH,NCO(aq)→(NH2)½CO(aq) the following data were obtained: [NH,NCO], M |0.715 8.95x10-2 1.05x103 0.358 0.179 minutes 150 449 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.715 M is min and when the starting concentration is 0.358 M is min. (2) The average A(1/[NHẠNCO]) / At from t= 0 min to t= 150 min i | The average A(1/[NH,NCO]) / At from t= 150 min to t= 449 min is M min. M' min!. (3) Based on these data, the rate constant for this | order reaction is M' min!.
5. What is the value for the rate constant, k? k = k'/1* = k = k"/0.5* = kavg r = k[OH°]*[ C25H3„N,'J" [OH] C2H,„N;'] r = 303