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For a second-order reaction, the rate constant k is the slope of the graph of 1/[A] versus t. Based on this information and the data given, calculate the rate constant k for the reaction. Express your answer in M−1⋅min−1 to three significant figures.

For a second-order reaction, the rate constant k is the slope of the graph of 1/[A] versus t. Based on this information and the data given, calculate the rate constant k for the reaction. Express your answer in M−1⋅min−1 to three significant figures.

Chemistry
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...
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Part B Please

 

Part A:

Consider the second-order reaction:

2HI(g)→H2(g)+I2(g)

Use the simulation to find the initial concentration [HI]0 and the rate constant k for the reaction. What will be the concentration of HI after t = 3.58×1010 s ([HI]t) for a reaction starting under the condition in the simulation?

Answer: 4.36×10−3 mol/L

Part B:

For a second-order reaction, the rate constant k is the slope of the graph of 1/[A] versus t. Based on this information and the data given, calculate the rate constant k for the reaction.
Express your answer in M−1⋅min−1 to three significant figures.
 
 
Most of the time, the rate of a reaction depends on the concentration of the reactant. In the case of Characteristics of second-order reactions second-order reactions, the rate is proportional to the square of the concentration of the reactant. For a second-order reaction, [A]→products, the rate of the reaction is given as rate = kA]², where k is the rate constant 1 = kt+ Select the image to explore the simulation, which will help you to understand how second-order reactions are identified by the nature of their plots. You can also observe the rate law for different and [A is the concentration of reactant A. The integrated rate law for second-order reactions is [A], where TAlo [At is the concentration of reactant A at time t, k is the rate constant, and Ao is the initial concentration of reactant A. This equation is of the type y = mx +b. Therefore, the plot of 1 versus time is always a straight line with a slope k and reactions. 1 a y intercept [A] (HI] mol/1 concentration, mol 1L [A]; mol 2H1 H; + : Rane lrw: N{HT -64-10 (mol s) 500 K Initial rate- 1.6-10' mol(]-s) 19 5 20 25 lime, 10s slope =k Start O Plet (1) vs. time O Piet InHT] vs. ime OPlet 1/THT) vs time Kese 1 [A]o In the simulation, you can select one of the three different kinds of plots. You may use the Start, Stop, and Reset buttons to observe the corresponding changes in the plot for different kinds of reactions. You can also select six different time, s reactions using the drop-down menu and observe three different types of plots for each reaction.
Transcribed Image Text:Most of the time, the rate of a reaction depends on the concentration of the reactant. In the case of Characteristics of second-order reactions second-order reactions, the rate is proportional to the square of the concentration of the reactant. For a second-order reaction, [A]→products, the rate of the reaction is given as rate = kA]², where k is the rate constant 1 = kt+ Select the image to explore the simulation, which will help you to understand how second-order reactions are identified by the nature of their plots. You can also observe the rate law for different and [A is the concentration of reactant A. The integrated rate law for second-order reactions is [A], where TAlo [At is the concentration of reactant A at time t, k is the rate constant, and Ao is the initial concentration of reactant A. This equation is of the type y = mx +b. Therefore, the plot of 1 versus time is always a straight line with a slope k and reactions. 1 a y intercept [A] (HI] mol/1 concentration, mol 1L [A]; mol 2H1 H; + : Rane lrw: N{HT -64-10 (mol s) 500 K Initial rate- 1.6-10' mol(]-s) 19 5 20 25 lime, 10s slope =k Start O Plet (1) vs. time O Piet InHT] vs. ime OPlet 1/THT) vs time Kese 1 [A]o In the simulation, you can select one of the three different kinds of plots. You may use the Start, Stop, and Reset buttons to observe the corresponding changes in the plot for different kinds of reactions. You can also select six different time, s reactions using the drop-down menu and observe three different types of plots for each reaction.
Examine experimental data Consider a second-order reaction in which reactant A decomposes according to the chemical equation 2A-products. The data given below is the time, in minutes, and the corresponding change in the concentration of reactant A for this reaction. t (min) [A](M) 0.00 0.500 20.0 0.382 40.0 0.310 60.0 0.260 80.0 0.224
Transcribed Image Text:Examine experimental data Consider a second-order reaction in which reactant A decomposes according to the chemical equation 2A-products. The data given below is the time, in minutes, and the corresponding change in the concentration of reactant A for this reaction. t (min) [A](M) 0.00 0.500 20.0 0.382 40.0 0.310 60.0 0.260 80.0 0.224
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