2) For a first order reaction the concentration of the reactant A changes with time according to the following table: t(s) [A] (M) 0 0.110 200 0.073 400 0.048 600 0.032 1000 0.014 A) Find the rate constant k graphically? Prove your answer mathematically? B) Find the concentration of A at 100 s graphically? Prove your answer mathematically?

2) For a first order reaction the concentration of the reactant A changes with time according to the following table: t(s) [A] (M) 0 0.110 200 0.073 400 0.048 600 0.032 1000 0.014 A) Find the rate constant k graphically? Prove your answer mathematically? B) Find the concentration of A at 100 s graphically? Prove your answer mathematically?

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

250 200 150 100 • (A] 50 0. 10 20 30 40 50 60 70 Time(s) (sec) The graph above shows concentration change over time for the following chemical reaction: Alg)- B(g) Which of the following statements is true about this reaction? The reaction is a first-order reaction. B) if the graph is replotted with 1/[A] versus time (t), the graph will be linear. C) The halfite of this reaction is constant. The first half-life of this reaction is 20 seconds. All of the above is not truti Concentration(M)
The graph below depicts the consumption of reactant A during a first-order reaction. (Enter all values to two significant figures.) [A], (M) 0.3 0.25 0.2 0.15 0.1 0.05 5 10 15 20 25 30 35 40 45 50 55 60 65 Using the graph, determine the half-life of the reaction. S (b) Calculate the rate constant and its units. ??? Time (s) Submit Answer
A chemistry graduate student is studying the rate of this reaction: 2C1,0, (g)- 2C1, (g) +50, (g) He fills a reaction vessel with Cl,0, and measures its concentration as the reaction proceeds: time [C,0,] (seconds) 0| 0.0900 M 10. 0.0579 M 20. 0.0372 M 30. 0.0239 M 40. 0.0154 M Use this data to answer the following questions. Write the rate law for this reaction. rate 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.
The following reaction was monitored as a function of time. 2H₂O₂ --> 2 H₂O + O₂ Time.(hr) [H₂O₂]. (M) 0 5.0 10.0 15.0 1.00 0.845 0.715 0.605 Which of the following statements is/are true? Multiple answers are possible. The general rate law for this reaction is rate = k[H₂O₂]². This reaction is first order in H₂O2. The rate constant is approximately 0.034. A plot of 1/[H2O2] versus time gives a straight line. This reaction is second order overall.
A student studies the concentration of reactant A over time in a reaction and gathers the following data. Use a spreadsheet program (or graph on paper) to determine the order of the reaction with respect to [A] and the rate constant. Enter the numeric value of the rate constant with at least 2 sig figs. time (sec) 0 34.6 82.3 103.1 142.2 179.7 230.0 [A]t [M] 1.146 0.984 0.794 0.708 0.558 0.413 0.233
T(K) k (M-¹s¹) Solve for the following: 400 8.10E3 C4H6 + C₂H4 → C6H10 500 42.4E3 600 128E3 The reaction order with respect to each reactant. Write your reasoning. The rate law for the reaction. 700 280E3
Please answer this question within 5 minutes, i will rate you for sure.
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
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]