**Rate Law for a Reaction Involving Reactant A**The rate law for a reaction is known to involve only the reactant A and is suspected to be either 1st or 2nd order.a. **Determine the Order of the Reaction**: You can determine the order of the reaction by measuring the time it takes for [A] to reach 50% and 25% of its original value, using the method of half-lives.b. **Determine the Rate Constant (k)**: To determine k for this reaction, you can sketch two plots (one for 1st order, one for 2nd order) with time on the x-axis and some form of [A] on the y-axis.**Explanation of the Plots**:- **First Order Reaction**: Plot ln[A] versus time. The plot should yield a straight line if the reaction is first order, and the slope will be equal to -k. - **Second Order Reaction**: Plot 1/[A] versus time. The plot should yield a straight line if the reaction is second order, and the slope will be equal to k.These visual representations help in identifying the order of the reaction and calculating the rate constant.

The half-life of a reaction is defined as the time taken for the initial concentration of the…

The rate law for a reaction is known to involve only the reactant A, and is suspected to be either 1st or 2nd order. Describe how the order of the reaction can be determined by measuring how long it takes for [A] to reach 50% and 25% of its original value (i.e., using the method of half-lives.) b. How would you determine k for this reaction? To help explain, sketch 2 plots (one for 1st order, one for 2nd) with time on the x-axis and some form of [A] on the y-axis. a.

The rate law for a reaction is known to involve only the reactant A, and is suspected to be either 1st or 2nd order. Describe how the order of the reaction can be determined by measuring how long it takes for [A] to reach 50% and 25% of its original value (i.e., using the method of half-lives.) b. How would you determine k for this reaction? To help explain, sketch 2 plots (one for 1st order, one for 2nd) with time on the x-axis and some form of [A] on the y-axis. a.

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

Give a clear handwritten answer with explanation....
1. The reaction 2A(g) A2(g) is being run in each of the following containers. The reaction is found to be second-order with respect to A. a. Write the rate law for this reaction. b. Which reaction container will have the greater reaction rate? c. In which container will the reaction have a shorter half-life? d. What are the relative rates of the reactions in each container? e. After a set amount of time has elapsed, which container will contain fewer A atoms?
7. The following data were obtained for the decomposition of N₂O5. a. Determine the reaction order with respect to N₂O5. b. Determine the rate constant for the reaction. Include units. c. Determine the concentration of N₂O5 after 3500 seconds. Time (s) 0 423 753 1116 1582 1986 2343 [N₂O5] (mol/L) 1.46 1.09 0.89 0.72 0.54 0.43 0.35
At a certain temperature the rate of this reaction is first order in Cl,0, with a rate constant of 0.0629 s 2C1,0; (3)– 2C1, (3) +50, (3) Suppose a vessel contains Cl,0; at a concentration of 1.01 M. Calculate how long it takes for the concentration of Cl,0; to decrease to 0.253 M. You may assume no other reaction is important. Round your answer to 2 significant digits.
11) the reaction A-→ B showed a second order kinetics. The rate constant, k for the reaction was found to be 0.964(I/mol.hr). If [A.) = 3.27 M. calculate the concentration of A that's left after 85.0 minutes a) 0.0122 M b) 1.67 M c) 0.598 M
Consider the mechanism. Step 1: B + C Step 2: E Overall: A + D B + E Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate = -kd[a] dt A C + D slow fast
#6 Q9
The half-life method determines the order of the reaction A -> products. Two setups were investigated, both at the same temperatures but with different initial concentrations of A. In the first run, the starting concentration of A was 0.78 M, and the half-life was determined to be 45 minutes. The initial concentration of A in the second run was 1.32 M. a. If the reaction is 0th order, what is the concentration of A in thesecond run after 152.3 minutes b. If the reaction is 1st order, what should be the half-life of the second run (minutes)? c. If the reaction is 2nd order, what should be the half-life of the second run (minutes)?
22.) A certain reaction has the rate law rate = k[A] where k = 0.539 min-1. How many minutes will it take for the [A] to decrease from 0.802 M to 0.299 M? Your Answer:
We are studying the reaction of 2A → 3B and we make a plot of ln[A] vs. time as the reaction proceeds. This plot turns out to be linear with a slope of -0.25 s-1.a. What is the value of the rate constant?b. What is the rate law expression for this reaction?
1. What is the significance of the order of the reaction? How does it affect the rate constant? 2. What are other ways to determine the temperature-dependence of a reaction? Explain the answers briefly.
3. Write the reaction rate equation and identify the order of reaction for the following equations: a. A + 2B b. 2N,O, c. Zn(s) +2HCI(aq)- 3C 4NO, + 0, → H,(g) + ZNCI, (aq)