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

Using the information in the table, the value of the rate constant for the reaction A(g) + 3 B(g) → C(g) + 2 D(g) is
The following initial rate data was obtained for the reaction between oxygen and nitric oxide. 2 NO(g) + O2(g) → 2 NO2(g) [O2] (M) [NO] (M) Rate (M s 1) 0.0100 0.0100 10.0 0.0150 0.0100 22.5 0.0150 0.0200 45.0 What is the rate law for this reaction under these conditions? Rate = k [O2] [NO]2 Rate = k [O2]2 [NO]2 Rate = k [O2] [NO] Rate = k [O2]² [NO]
Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 0.496M 1.63 M 6.00 × 10³ M/s 0.496M 0.191M 82.4M/s 0.209M 1.63 M 2.53 × 10³ 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 = | x10 ロ・ロ X
For the given equation at 800 °C: CO(g) + Ch(g) > COCh(g), the following data were collecica Experiment (COL(M) 0.96 1.92 0.96 (CH] (M) 1.60 1.60 3.20 Rate of appearance COCh (M/s) 0.121 0.242 0.484 Determine the Rate Law for the reaction From your Rate Law determined in question #1 above, determine the value of the rate constant WITH THE APPROPRIATE UNITS. ONLY If you could not answer #1 above, use this "mock" data to solve for k: Rate = K[ARB]?, with [A] = 1.00 M and B]o = 1.50 M, with a rate of 2.50 x 10-2 M/s.
Which of the following statements about rate laws is FALSE? A) Rate laws can only be determined experimentally. B) Rate laws tell us information about the mechanism of the chemical reaction under study. C) The rate law for the chemical reaction A + B + 20 –D must be rate = k[A][B][C]² %3D D)A rate law can only be written for the elementary reactions of a given chemical reaction.
just need standard error for K
Consider the reaction: A + B --> products. From the following data obtained at a certain temperature, determine the order of the reaction (rate law) and calculate the rate constant: [A] (M) [B] (M) Rate (M/s) 1.50 1.50 3.15 X 10-1 1.50 2.50 2.98 X 10 –1 3.00 1.50 5.50 X 10-1
A + B +C → D Reaction [A] (М) [B] (М) [C] (М) Experiment Rate () 0.10 0.10 0.10 0.003 2 0.20 0.10 0.10 0.012 3 0.10 0.30 0.10 0.003 4 0.20 0.10 0.20 0.024 Determine the rate of the reaction when [A]= 0.30 M, [B] = 0.10 M and [C] = 0.20 M.
or a reaction involving two reagents A and B, the following data was collected over three experiments. Exp# [A] [B] Rate (M/s) 1 0.20 M 0.20 M 5.0 2 0.20 M 0.40 M 20.0 3 0.10 M 0.40 M 10.0 Using the above data, which of the following is the rate law for the reaction of A with B?
The concentration of A was monitored for the reaction A → P and the following data were obtained. What is the rate law, rate = k [A]x, for this reaction? [A] (M) Time (s) 0.0200 0 0.0169 100 0.0142 200 0.0120 300 0.0101 400 0.0086 500 0.0072 600 0.0061 700 Question 15 options: rate = 1.7 x 10–3 [A] rate = 2.3 x 10–3 [A]2 rate = 0 54 [A] rate = 1.3 x 10–3 [A] rate = 0 54 [A]2
A chemistry graduate student is studying the rate of this reaction: →H2CO3aq+H2OaqCO2aq She fills a reaction vessel with H2CO3 and measures its concentration as the reaction proceeds time(seconds) H2CO3 0 0.500M 10. 0.101M 20. 0.0563M 30. 0.0390M 40. 0.0298M Use this data to answer the following questions. Write the rate law for this reaction. rate =k 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. =k
The following graph displays the concentration of bromine gas during the reaction H₂(g) + Br₂(g) →2HBr(g). Concentration (M) 1.2- 1.0 0.8 0.6- 0.4 0.2- 0+ [Br₂] 50 Time (s) On a separate sheet of paper, determine the following quantities and upload a picture of your work for credit: a) the average rate of the reaction between Os and 25s. b) the instantaneous rate of the reaction at 25s c) the instanteous rate of the formation of HBr at 50s 100 150