P17B.4 The data below apply to the reaction, (CH,),CBr(aq) + H,0(1) → (CH,),COH(aq) + HBr(aq). Identify the order of the reaction and calculate the rate constant and the molar concentration of (CH,),CBr remaining after 43.8h. t/h 3.15 6.20 10.00 18.30 30.80 [(CH,),CBr]/(10²mol dm³) 10.39 8.96 7.76 6.39 3.53 2.07

P17B.4 The data below apply to the reaction, (CH,),CBr(aq) + H,0(1) → (CH,),COH(aq) + HBr(aq). Identify the order of the reaction and calculate the rate constant and the molar concentration of (CH,),CBr remaining after 43.8h. t/h 3.15 6.20 10.00 18.30 30.80 [(CH,),CBr]/(10²mol dm³) 10.39 8.96 7.76 6.39 3.53 2.07

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

18.) A generic reaction has the rate law rate = k[A]2[B]1. What is the value of the rate constant, k, if the rate = 0.517 M/s when the [A] = 0.413 M and [B] = 0.904 M? Do not include units. Your Answer:
The decomposition of [A] in solution at 75C proceeds via first order: A (aq) yields B (aq) What is the rate law for the reaction?
The following kinetic data were collected at 298 K for the reaction of ozone with nitrite ion, producing nitrate and oxygen: NO, (aq) +O,(g) NO, (aq) +0,(g) > Experiment [NO2 lo (M) [O3lo (M) Initial Rate (M/s) 1 0.0100 0.0050 25.0 0.0150 0.0050 37.5 3 0.0200 0.0050 50.0 0.0200 0.0200 200.0
The following data were obtained for the reaction 2A → B: Time, min TA], mol/L 0.0962 0.0398 0.0156 10 20 40 60 80 0.0059 0.000428 0.000061 0.000009 (i) By plotting a suitable graph, determine the order of this reaction. (i) Calculate the rate constant of the reaction.
Q2) Calculate the rate constant for the first order decomposition reaction of phosphine [PH3], M (at 120 °C): 4PH3(g)→ P4(g) + 6H₂(g)? .64 * 10 ^ - 2 Time (sec) a) 2.47 * 10 ^ - 2 * s ^ - 1 0 2.32 *10^ - 8 1.16 * 10 ^ - 2 (5.80 * 10 ^ - 3)/84 b) 28s ^ - 1 c) 4.64*10^ -2 overline s^ -1 56 d) 3.57 * 10 ^ - 2 * s ^ - 1
The rate law for the reaction A2BM2(aq) + 2A(aq) + 2D(aq) → D2(aq) + 2A½Bm (aq) is rate = k(A2Bm2)(D). %3D What is the overall order of the reaction? O zeroth order O first order third order second order
Fe3+ (aq) + 7.00 SCN- (aq) → Fe(SCN)7.00 3+ (aq) 1.)Find the rate where SCN- is consumed, if Fe3+ is consumed at 1.00 M/min. 2.) Find the rate and the overall order of the rate law
Be sure to answer all parts. Consider the reaction A+BProducts From the following data obtained at a certain temperature, determine the order of the reaction. Enter the order with respect to A, the order with respect to B, and the overall reaction order. A. JA] (M) (BỊ (M) Rate (Mis) 1.50 1.50 3.20 x 10 1.50 2.50 3.20 x 10 Reaction 3.00 1.50 6.40 x 10
Consider the hypothetical reaction A(g) + B(g) C(g) The four containers below represent this reaction being run with different initial amounts of A and B. Assume that the volume of each container is 1.0L. The reaction is second order with respect to A and first order in respect to B. Which of the containers, W,X,Y or Z, would have the greatest reaction rate? Justify your answer.
Consider the mechanism. Step 1: Step 2: А +В — С slow А +С — D fast Overall: 2A + В — D Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate =
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0022 M⚫s 1: 2 HI (g) →H₂ (g) +12(g) Suppose a 4.0 L flask is charged under these conditions with 250. mmol of hydrogen iodide. How much is left 7.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. X x10
6) For the process at 0.00 oC: 2 NO2 (g) à N2O4 (g) , the rate constant is 4.18 x 10–6 M–1s–1. How many hours will it take for 18.0 % NO2 to be remaining? a) 36.2b) 10.8 c) 303 d) 125 e) 78.7 f) 14.6