A study of the rate of the reaction represented as 2A → B gave the following data: Time (s) 0.0 5.0 [A] (M) 1.00 0.775 0.625 0.465 0.360 || 0.285 || 0.230 Determine the average rate of disappearance of A between: 0.0s and 10.0 s M/S and between 10.0 s and 20.0 s M/S 10.0 15.0 20.0 25.0 35.0

A study of the rate of the reaction represented as 2A → B gave the following data: Time (s) 0.0 5.0 [A] (M) 1.00 0.775 0.625 0.465 0.360 || 0.285 || 0.230 Determine the average rate of disappearance of A between: 0.0s and 10.0 s M/S and between 10.0 s and 20.0 s M/S 10.0 15.0 20.0 25.0 35.0

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

Please don't provide handwritten solution ...
The rate constant for a reaction is found to be 0.15 M-1s-1. If the initial concentration of the reactant is 0.20 M, how long (in seconds) does it take for the concentration to decrease to 0.15 M?
The following initial rate data are for the reaction of ICI with hydrogen: 2 ICI + H2- →I2 + 2 HCI Experiment [ICI],, M [H2]o, M Initial Rate, M s-1 1 0.339 7.80x10-2 |3.63х10-3 0.678 7.80x10-2 7.26x10-3 3 0.339 0.156 1.45x10-2 14 0.678 0.156 2.90x10-2 Complete the rate law for this reaction in the box below. Use the form k[A]m[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 M-2s-1.
6. The following data were obtained for the reaction: A → products. Determine the rate law for this reaction, including the value of k. [A] (M) time (s) 0.800 0 0.775 40 0.750 83 0.725 129 0.700 179
Given the information based on time and concentration, determine the order of the reaction and the rate constant k when graphing the following data: A--> C+D Time (s) (A] M 10 0.1000 50 0.0856 100 0.0749 200 0.0598 350 0.0460 500 0.0373 800 0,0271
A certain reaction is first order in N, and second order in H,. Use this information to complete the table below. Be sure each of your answer entries has the correct number of significant digits. [N] [4.] initial rate of reaction x10 1.91 M 0.885 M 0.894 M/s olo 0.813 M 0.885 M I|| M/s Ar 0.213 M 7.92 M
A chemistry graduate student is studying the rate of this reaction: 2H1 (g) - H₂ (g) +1₂ (g) She fills a reaction vessel with HI and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 [HI] 1.00 M 0.227M 0.20 0.128M 0.30 0.0894M 0.40 0.0686M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate=& D.D
Determine the rate of the reaction at t = 35s for the following reaction: C2H2(g) + O3(g) → C2H4O(g) + O2(g), suppose the following concentration vs. time data were collected: Time, s [O3(g)], mol L-1 0 3.20x10-5 10 2.42x10-5 20 1.95x10-5 30 1.63x10-5 40 1.40x10-5 a. 4.3 × 10-7 mol L-1s-1 b. 5.3 × 10-7 mol L-1s-1 c. 2.3 × 10-7 mol L-1s-1 d. 7.3 × 10-7 mol L-1s-1
For the reaction A → products, concentration and time data were collected. t (s) [A] (M) Enter these data into the graphing tool to determine the reaction order. 0.0 3.40 25.0 2.28 50.0 1.53 75.0 1.02 Graphing Tool Clear All Data [A] vs. t In[A] vs. t 1/[A] vs. t t [A] In[A] 1/[A] 3.4 3.4 1.223775 0.294118 25 2.28 0.824175 0.438596 2.822 + 50 1.53 0.425268 0.653595 2.244 + 75 1.02 0.019803 0.980392 1.666 - 1.088 - 0.51 - 15 30 45 60 75 t y=-0.03156 x + 3.241000 2= 0.971 Add Row 10 total rows What is the reaction order? O 1 Calculate the concentration of A after 127 s. [A]127 s = M [V)
The following kinetic data were obtained for the reaction A (g) + 2 B (g) → products Trial [A] (M) [B] (M) Initial Rate (M s-1) 1 0.60 0.30 0.0126 2 0.20 0.30 0.0014 3 0.60 0.10 0.0042 Determine the order with respect to A. Enter the answer as a single digit, not the word.
Given below is the data for the reaction. Calculate the value of the rate constant "k" with proper units. A + B → C Set [A] (M) [B] (M) Init, rate M-sec 1 0.050 0.200 5.0 x 10-5 2. 0.100 0.200 5.0 x 10-5 0.050 0.600 4.5 x 10-4 Determine the order in "A" Determine the order in "B" Substitute the order for A and B in the rate law equation below. Rate = k [A]' [B]