Еxperiment[A]o (M)[B], (M)Rate (M/s)10.01000.1001.0 X 10-030.03000.1003.0 × 10–030.03000.3002.7 × 10–02a) Determine the rate law for this reaction.b) Calculate the rate constant.c) Calculate the rate when [A] 0.200 M and [B] 0.200 M.6. A reaction of the form aA → Products is second order with a half-life of 425 s. What is the rate constant of thereaction if the initial concentration of A is 5.99 x 10° mol/L?7. The following values of the rate constant were obtained for the decomposition of nitrogen dioxide at varioustemperatures. Plot the logarithm of k versus 1/T and from the graph obtain the energy of activation.Тетрerature ( C)k (L/mol s)3200.5273300.7763401.1213501.607Topic: Nuclear chemistry8. Complete the following nuclear reactions.a. Sib. STi + ?ISP + ?>442244--21142-56252,C. 98CFBa + ? + 4on>9. Consider Rn-222a. Predict the type of radioactive decay that Rn-222 is most likely to undergo.b. Write the equation for the decay process.c. The half-life of Rn-222 is 3.82 days. If you start with a 150.0-g sample of Rn-222, how much remains after15.0 days?

Since you have posted a question with multiple sub-parts, we will solve the first three subparts for…

Еxperiment [A], (M) [B], (M) Rate (M/s) 1 0.0100 0.100 1.0 × 10¬03 2 0.0300 0.100 3.0 × 10–03 3 0.0300 0.300 2.7 × 10¬02 a) Determine the rate law for this reaction. b) Calculate the rate constant. c) Calculate the rate when [A] 0.200 M and [B] 0.200 M.

Еxperiment [A], (M) [B], (M) Rate (M/s) 1 0.0100 0.100 1.0 × 10¬03 2 0.0300 0.100 3.0 × 10–03 3 0.0300 0.300 2.7 × 10¬02 a) Determine the rate law for this reaction. b) Calculate the rate constant. c) Calculate the rate when [A] 0.200 M and [B] 0.200 M.

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

Pure ozone decomposes slowly to oxygen, 203(g) – 30,(g). Use the data provided in a graphical method and determine the order and rate constant of the reaction. Time (h) 2.0 x 103 7.6 x 103 1.00 x 104 [0] (M) 1.00 x 10-5 4.98 x 10-6 2.07 x 10-6 1.66 x 10-6 Time (h) 1.23 x 104 1.43 x 104 1.70 x 104 [O3] (M) 1.39 x 10-6 1.22 x 10-6 1.05 x 10-6
Using the data in the table, determine the rate constant of the Trial [A] (M) [B] (M) Rate (M/s) reaction and select the appropriate units. 1 0.200 0.400 0.0155 2 0.200 0.800 0.0155 A + 2B » C+ D 3 0.400 0.400 0.0620 Units k =
Consider the data table below for the generic reaction A + B → products Trial [A] (M) [B] (M) Rate (M/s) 1 0.150 0.100 9.00×10−4 2 0.150 0.200 1.80×10−3 3 0.300 0.100 3.60×10−3 4 0.600 0.200 2.88×10−2 Determine the rate law for the reaction. (You do not need to calculate ) Show your work or explain your reasoning. What are the units of and how do you know?
The following data were collected for this reaction: 2NO2(g) + 2F2(g) > 2NO2F(g) [NO2] [F2] [2NO2F] 0.100 0.100 0.026 0.200 0.100 0.051 0.200 0.200 0.103 0.400 0.400 0.411 A) Write the expression for the reaction rate law B) Find n value for [NO2] C) Find m value for [F2] D) Calculate the k value of k for this reaction
Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.88M 1.34M 52.0 M/s 1.88M 0.296M |0.514M| 1.34M rate = k Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. k = 11.5 M/s 0 3.89 M/s x10 0.0 X
Deducing a rate law from the change in concentration over time A chemistry graduate student is studying the rate of this reaction: 2C1,0, (g) → 2C1, (g) + 50, (g) He fills a reaction vessel with Ci,0, and measures its concentration as the reaction proceeds: time [C1,0,] (seconds) 0.0500M 10. 0.0170M 20. 0.0103 M 30. 0.00735 M 40. 0.00573 M Use this data to answer the following questions. Write the rate law for this reaction. rate = k Calçulate the value of the rate constant k. k = Round your answer to 2 significant digits. Also be ? sure your answer has the correct unit symbol.
Determine the rate law and the rate constant for this reaction. 13.125. The table contains reaction rate data for the reaction 2 NO(g) + Cl,(g)→ 2 NOCI(g) Initial Rate Experiment [NO], (M) [Cl_]o (M) (M/s) 1 0.20 0.10 0.63 0.20 О.30 5.70 0.80 0.10 2.58 0.40 0.20 Predict the initial rate of reaction in experiment 4. 13.126. An important reaction in the formation of photochemical smog is the reaction between ozone and NO: NO(g) + O3(g) → NO;(g) + O,(g) 2. 2. 3.
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:
Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. [H₂] [2] initial rate of reaction 1.96M 1.54M 0.939 M 1.54M 1.96M 0.618M 4.00 × 104 M/s 1.92 × 10 M/s 1.61 × 104 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k] k = 0 □·□ 吕
Some measurements of the initial rate of a certain reaction are given in the table below. [N-] N2 H2 initial rate of reaction 0.556M 1.54M 6.00 × 10°M/s 0.181 M| 1.54M 1.95 × 10°M/s 0.556M 2.66M 1.79 × 10°M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k U x10 k =
Consider the following reaction. Calculate the value of the rate constant.. 3 A + B → 2 C Trial [A]0 [B]0 [C]0 Rate (M/s) 1 0.61 0.15 0.071 3.013 2 1.22 0.15 0.071 12.052 3 0.61 0.3 0.071 12.052 4 0.18 0.78 0.071 ?
2 NO(g) + Br2 (g) → 2 NOB1(g) Initial Rate Experiment NO] (M) [Br2] (M) (mol/L's) 1 1.0 x 10-2 2.0 × 10-2 2.4 x 10-2 2 4.0 x 10-2 2.0 × 10-2 0.384 3 1.0 x 10-2 6.0 x 10-2 7.2 x 10-2 What is the order of the reaction with respect to [NO] and [Br2], and what is the overall order of the reaction? Order with respect to [NO] = Order with respect to [Br2] = Overall order