by measuring the concentration of A every 30 seconds. The student plots the results. Theplot is shown below. What is the rate constant for the reaction?In [A] In (M)-12.0-12.5-13.0-13.514.0-14.5-15.0-15.5-16.0O0y = -0.0032x-13.165200400time (sec)A) -0.0032 sec-1B) -13.165 sec-1OC) 13.165 sec-1D) 0.0032 sec-1600800

by measuring the concentration of A every 30 seconds. The student plots the results. The plot is shown below. What is the rate constant for the reaction? -12.0 -12.5 -13.0 -13.5 S-14.0 -14.5 -15.0 -15.5 -16.0 0 y = -0.0032x-13.165 200 400 time (sec) OA) -0.0032 sec¯1 O B) -13.165 sec¯1 OC) 13.165 sec-1 D) 0.0032 sec-1 600 800

by measuring the concentration of A every 30 seconds. The student plots the results. The plot is shown below. What is the rate constant for the reaction? -12.0 -12.5 -13.0 -13.5 S-14.0 -14.5 -15.0 -15.5 -16.0 0 y = -0.0032x-13.165 200 400 time (sec) OA) -0.0032 sec¯1 O B) -13.165 sec¯1 OC) 13.165 sec-1 D) 0.0032 sec-1 600 800

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

Consider the plot that shows the concentration of the reactant A in the reaction A → B. Which expression would you use to find the average rate of the reaction between 10 and 20 seconds? 1.2 0.8 [A] 0.6 0.4 - 0.2 0- O 10 20 30 40 50 60 70 80 Time (s) O (0.75M-0.85M)/(20s-10s) -(0.75M-0.85M)/(20s-10s) -(0.85M-0.75M)/(20s-10s) O -(0.85M-0.75M)/(10s-20s) Concentration (M)
Given the information below, determine the rate law for the reaction and the rate constant (k). Be sure to include the units for the rate constant (k). A + 2B --> C + D [A] M [B] M Initial Rate (M/s) 0.10 0.10 0.0015 0.20 0.10 0.0060 0.20 0.20 0.0120 0.40 0.10 0.0240 rate law: rate constant k:
Can someone help me with this problem. I tried it out but I know you cannot have negative K value.
None
For A products, time and concentration data were collected and plotted as shown. [A] (M) t (s) 0.900 00.0 0.474 30.0 0.321 60.0 0.243 90.0 t Determine the reaction order, the rate constant, and the units of the rate constant. order= *k = [A] MacBook Pro In[A] t (units) 1/[A] t
A chemistry graduate student is studying the rate of this reaction: 2N,0, (g) 2N,04 (g) +0, (g) He fills a reaction vessel with N,O, and measures its concentration as the reaction proceeds: time [N,0,] (milliseconds) 1.00M 10. 0.504M 20. 0.337M 30. 0.253 M 40. 0.203 M
The rate of a certain reaction was studied at various temperatures. The table shows temperature (?) and rate constant (?) data collected during the experiments. Plot the data to answer the questions. What is the value of the activation energy, ?a , for this reaction? ? (?) ? (?−1) 400 0.000659 420 0.00327 440 0.0181 460 0.0589 480 0.213 500 0.615 520 1.66 540 3.99 560 9.64 580 20.1 Ea= What is the value of the pre‑exponential factor (sometimes called the frequency factor), ? , for this reaction?
A scientist evaluated reaction rates for the reaction A + B --> C using differing initial concentrations of A and B and collected the following data: [A] [B] Rate 0.492 0.430 2.339 0.492 0.860 4.678 0.984 0.430 9.356 0.984 0.860 18.712 a) What is the rate order for reactant B in the rate law for this reaction?
A chemistry graduate student is studying the rate of this reaction: 2C1₂05 (g) → 2Cl₂(g) +50₂ (g) She fills a reaction vessel with Cl₂O5 and measures its concentration as the reaction proceeds: time (minutes) 0 10. [CI,Os] 0.300M 0.161M 20. 0.0864M 30. 0.0464M 40. 0.0249M 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 = k k = x10 0.0 X 5
which answer is correct?
For the reaction of : 2 H2O2 (g) → 2 H2O (g) + O2 (g), consider this data table, What is the average rate of reaction between 40 and 50 s for hydrogen peroxide? Time (s) H2O2 (M) 0 1.000 10 0.747 20 0.561 30 0.403 40 0.298 50 0.214 -0.0084 M/s 0.0042 M/s 0.0168 M/s 0.214 M/s 0.0084 M/s
Given the following information about a reaction with a reactant A: Time (s) 0.0 6.0 12.0 18.0 [A](M) 1.22 0.61 0.31 0.15 What is the initial rate of the reaction (rate from 0.0 s - 6.0 s)?