5. The reaction A products is a second-order reaction and takes place at 32°C. a. Given that the half-life of this reaction is 4.22 x 104 s when the initial concentration of A is 0.2 M, what is the rate constant for the reaction? Include units with your answer. b. At 305 K, how long will it take for a 0.028 M sample of A to decrease to 0.0042 M? c. Initially 4.00 mol of A is placed in a 6.00 L container and allowed to react. How many moles of A would remain after 24.0 hours? Assume the temperature is 32 °C.

5. The reaction A products is a second-order reaction and takes place at 32°C. a. Given that the half-life of this reaction is 4.22 x 104 s when the initial concentration of A is 0.2 M, what is the rate constant for the reaction? Include units with your answer. b. At 305 K, how long will it take for a 0.028 M sample of A to decrease to 0.0042 M? c. Initially 4.00 mol of A is placed in a 6.00 L container and allowed to react. How many moles of A would remain after 24.0 hours? Assume the temperature is 32 °C.

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

Related questions

Q: At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.154M…

A: The given chemical reaction is as follows:The rate constant for the second order reaction = The…

Q: The following problems require graphing. You may do this by hand or using the spreadsheet on Google…

A: Rate constant is the proportionality constant when rate of reaction is directly proportional to…

Q: A second-order reaction starts with an initial concentration of 0.5 mol/L of the reactant. If the…

A: Given data contains, Initial concentration of the reactant is 0.5 mol/L. Final concentration of the…

Q: The decomposition of SO,Cl, is first order in SO,Cl, and has a rate constant of 1.42 x 10-ts-1 at a…

A: The half-life of a reaction is defined as the time required for a reactant to be decreased to half…

Q: 1. 2NO(g) + Cl₂(g) The following data were collected for the reaction above. Initial [NO] (M)…

A: Note : Dear student since you have posted multiple parts question, as per bartleby qna guidelines we…

Q: . A student graphed the natural log of concentration versus time and obtained a straight line. The…

Q: The decomposition of sulfuryl chloride, SO,Cl2, is a decomposition at 660 K is 4.5x10²s. The initial…

A: Given initial pressure is 450 torr

Q: The following reaction: CH3CH₂Br + H₂O CH3CH₂OH + HBr is first order with respect to CH3CH₂Br and…

Q: Calculate the rate constant (in units M/min) for a zero order reaction

A: Given : t1/2 = 82.4 min [A]o=0.787 M To calculate : rate constant (k)

Q: Graph the following data for the first-order decomposition reaction of N₂O5 as [N₂Os] vs time (y vs…

A: The concentration of the and the time are as follows:Conce. of time…

Q: 3.) NO2 decomposes to yield NO and O2 according to the equation given below. The reaction is second…

Q: The decomposition of gaseous dinitrogen pentaoxide (N2O5) to NO2 and O2 is a first-order reaction.…

Q: Cyclobutane decomposes when heated in a first order reaction to give ethylene by the reaction shown…

Q: The following reaction was determined to be elemtary: A + 2B -> C What is the overall of the…

Q: The rate constant for this second-order reaction is 0.560 M-1 •s-1 at 300 °C. A → products How long,…

Q: . A reaction that is second-order in one reactant has a rate constant of 2.2 x 10-2 L/(mol • ). If…

A: Given : Rate constant of reaction = 2.2 X 10-2 M-1s-1. Initial concentration of reactant = 0.360 M…

Q: It is found that a gas undergoes a zero order decomposition reaction in the presence of Ni catalyst.…

Q: Answer the following questions regarding the first order decomposition of dinitrogen pentoxide at…

Q: The kinetics of this reactant were studied as a function of temperature. (The reaction is first…

A: The rate is directly proportional to the square of reactant concentration is known as second order…

Q: Molecular iodine, I2(g), dissociates into iodine atoms at 625 K with a first-order rate constant of…

Q: The reaction of nitric oxide with hydrogen at 1280°C is: 2 NO(g) + 2 H2(g) → N2(g) + 2 H₂O(g) From…

Q: At 330 degrees Celsius, the rate constant for the second order decomposition of NO2 is 0.775M ^ - 1…

Q: 5. A laboratory experiment was done for the reaction below and the following data was obtained: A→…

A: The objective of this question is to determine the order of the reaction and the reaction rate…

Q: The following data were obtained from a study of the decomposition of CHEM at 320 oC: t, seconds…

A: A question based on Chemical kinetics. A set of data for the decomposition of CHEM at 320°C is…

Q: What is the overall order of the reaction? b. Write the rate expression. c. Calculate the rate…

A: A. We have to calculate the overall order . B.rate expression has to be written. C. Rate constant…

Question

100%

5. The reaction A products is a second-order reaction and takes place at 32°C.
a.
Given that the half-life of this reaction is 4.22 x 104 s when the initial concentration of A is 0.2 M, what is
the rate constant for the reaction? Include units with your answer.
b. At 305 K, how long will it take for a 0.028 M sample of A to decrease to 0.0042 M?
c. Initially 4.00 mol of A is placed in a 6.00 L container and allowed to react. How many moles of A would
remain after 24.0 hours? Assume the temperature is 32 °C.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

15. The decomposition of sulfuryl chloride (SO2Cl2) is a first-order process. The rate constant for the decomposition at 660 K is 4.5 10-2 s-1.By what factor will the pressure of sulfuryl chloride decrease after 6 half-lives? Note: The answer wants this value: (360. torr)/value = final pressure after decay _______ value
Consider the reaction A > B. The initial [A] is 0.10 M. After 1.0 hour, 50% of A has reacted. a. Draw a graph of concentration vs. time for each of the cases below. i. The reaction is zero order in A. I. The reaction is first order in A. b. Predict what the concentration of A will be after 2.0 hours for each case in part a if the initial [A] were 0.050 M. Explain your reasoning.
The reaction between hydrogen and chlorine is as follows: Cl2(g) + H2(g) → 2HCl(g) Experiments show that this reaction is first order with respect to H2 and one-half order with respect to Cl2. What is the rate law? a. Rate = k [H2]1/2 [Cl2] b. Rate = k [Cl2] [H2]2 c. Rate = k [Cl2]1/2 [H2] d. Rate = k [Cl2]2 [H2]
Molecular iodine, I2 (g), dissociates into iodine atoms at 652 K, with a first order rate constant of 0.452 s-1. I2(g) -----> 2I a. What is the half life for this reaction? b. If you start with 0.35 M I2 at this temperature, how long will it take for the concentration of I2 to reach 0.12 M?
For the reaction below, a series of experiments was conducted and the data collected in the table below. a. Determine the rate law and the overall order of the reaction. b. Calculate the rate constant, including appropriate units. c. Determine the initial rate when the initial concentrations of both reactants are 0.12 M. Reaction (might be unbalanced): NO (g) + Cl2 (g) → NOCI (g) Experiment Data: Experiment # Initial [NO] (M) Initial [Cl2] (M) Initial Rate (M/s) 0.13 1.0x10-2 0.20 2 0.26 0.20 4.0x10-2 3 5.0x10-3 0.13 0.10
The reaction of 2 N2O5(g) → 4 NO2(g) + O2(g) is experimentally determined to be fırst oder. What experimental data would support this conclusion? I. Plotting 1/[N2O5] vs. time would be linear. II. The half-life is independent of the initial concentration. III. Doubling the initial concentration of N205 would yield a quadrupled initial rate. Only I. Only II. II. and III. I. and III.
Which one of the following statements is correct? O A. At eguilibrium, the rates of the forward and reverse reactions are both zero. B. The units of a reaction rate depend on the overall order of the reaction. C. Rates of catalyzed chemical reactions do not depend on temperature. O D. The half-life for a second-order reaction of the type A → products remains constant over time. E. The rate of a first-order reaction decreases with time.