**Topic: Reaction Kinetics and Rate Laws***Overview:*Nitrosyl bromide decomposes by the reaction \( 2 \text{NOBr}(g) \rightarrow 2 \text{NO}(g) + \text{Br}_2(g) \). The objective is to show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction.*Data Presentation:*- The reaction data can be analyzed by plotting the data in three different ways.- For each plot, time \( t \) goes on the x-axis.- A zero-order reaction is linear when \([\text{NOBr}]\) is on the y-axis.- A first-order reaction is linear when \(\ln([\text{NOBr}])\) is on the y-axis.- A second-order reaction is linear when \(1/[\text{NOBr}]\) is on the y-axis.*Given Data:*\[\begin{array}{c|cccccc}t \text{ (s)} & 0 & 5 & 10 & 15 & 50 & 85 \\\hline[\text{NOBr}] \text{ (M)} & 0.0653 & 0.0514 & 0.0424 & 0.0361 & 0.0177 & 0.0117 \\\end{array}\]*Questions:*1. What is the rate law for the reaction? (Rate equations take the general form 'rate = k \cdot [A] \cdot [B]^n'.) - The reaction is determined to be second order, indicated by a linear plot of \(1/[\text{NOBr}]\) vs. time.2. What is the value of the rate constant at the temperature of the experiment? - The rate constant \( k \) is given as 49.0.3. What are the units for the rate law? - Options provided: - \( \text{M}^{-2} \cdot \text{s}^{-1} \) - \( \text{M}^{-3} \cdot \text{s}^{-1} \) - \( \text{M}^{-2} \cdot \text{s}^{-2} \) - \( \text{

In order to find the order of the reaction, we have to plot 3 different graphs. The graph having the…

Nitrosyl bromide decomposes by the reaction 2 NOBr(g) → 2 NO(g) + Br₂(g). Show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction. Students may do this by plotting the data three different ways. For each plot, time goes on the x-axis. zero-order reaction is linear when [NOBr] on the y-axis. first-order reaction is linear when In[NOBr] is on the y-axis. second-order reaction is linear when 1/[NOBr] is on the y-axis. t 0 5 10 15 50 85 [NOBr] 0.0653 0.0514 0.0424 0.0361 0.0177 0.0117 M What is the rate law for the reaction? (Rate equations take the general form 'rate = k. [A]. [B]'.) What is the value of the rate constant at the temperature of the experiment? What are the units for the rate law? OM-2.5-1 OM-3.5-1 OM-².5-2 O M-1. s-1 chemPad XX→ ← Help Greek

Nitrosyl bromide decomposes by the reaction 2 NOBr(g) → 2 NO(g) + Br₂(g). Show that the following data are consistent with a second-order reaction and determine the second-order rate constant for the reaction. Students may do this by plotting the data three different ways. For each plot, time goes on the x-axis. zero-order reaction is linear when [NOBr] on the y-axis. first-order reaction is linear when In[NOBr] is on the y-axis. second-order reaction is linear when 1/[NOBr] is on the y-axis. t 0 5 10 15 50 85 [NOBr] 0.0653 0.0514 0.0424 0.0361 0.0177 0.0117 M What is the rate law for the reaction? (Rate equations take the general form 'rate = k. [A]. [B]'.) What is the value of the rate constant at the temperature of the experiment? What are the units for the rate law? OM-2.5-1 OM-3.5-1 OM-².5-2 O M-1. s-1 chemPad XX→ ← Help Greek

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

A decomposition reaction follows second order kinetics with a rate constant, k = 0.0137 M-1 min-1. If the initial concentration of the reactant is 0.866 M, what is the concentration after 5 minutes? Report your answer to the thousandths place and do not include units.
The decomposition of compound XYZ is a 2nd order reaction. Initially, the concentration of XYZ was 2.80 M. If the rate constant of this reaction is 4.31 M-1 min-1. How many minutes are required for the concentration of XYZ to become 0.700 M? Your answer should have 3 significant figures.
The decomposition of aqueous hydrogen peroxide in a given concentration of catalyst yielded the following data: [H, O2] 0.1000 M 0.0804 M 10.0 min 0.0648 M Time 0.0 min 5.0 min 15.0 min 0.0519 M Verify that the reaction is first-order. Determine the rate constant for the decomposition of H2 O2 (in units of /s) from the slope of the straight-line plot of In H2O2] versus time.
The table gives the concentrations of C₂H₂O(g) as a function of time at a certain temperature for the reaction shown. C,H,Og) —CH,(g)+CO(g) Verify that this is a first-order reaction by plotting In[C,H,O] versus time and determining the value of the rate constant. [C₂H4O] (M) 0.0860 0.0465 0.0355 0.0274 0.0174 Time (min) 0.00 50.0 72.0 93.0 130.0 min
The following data show the rate constnat of a first order reaction measured at several different temperatures. Construct and Arrhenius plot (ln k vs 1/T) to determine the activation energy (Ea). You should use a graphing program like excel to construct your graph. A sketch of the graph including the equation of the line should be included in your notebook. temperature (K) rate constant (s-1) 375 1.68 x 10-5 400 3.50 x 10-5 500 4.20 x 10-4 600 2.11 x 10-3
The half-life of a first-order reaction is found to be 28.25 min.What is the value of the rate constant for this reaction?If a 1.00 g sample of reactant is used, what mass will remain after 45 minutes?
Consider a first-order decomposition of the substance A. It takes 60 min ufor the concentration of A to drop to half its initial value. How long, in total, will it take for the concentration of A to fall from its initial value to 12.5%? Select one: 1. 45 min 2. 15 min 3. 180 min 4. 120 min 5. None of the other answers
A certain first-order reaction is 61 percent complete in 65 seconds. Calculate the rate constant for this reaction.
It has been found that DDT in the soil decomposes by a first-order reaction with a half-life of 12.0 years. How long would it take DDT in a soil sample to decompose from a concentration of 165 ppbm (parts per billion by mass) to 15 ppbm?
At a certain temperature this reaction follows first-order kinetics with a rate constant of :0.0303s−1 →NH4OHaq+NH3aqH2Oaq Suppose a vessel contains NH4OH at a concentration of 0.410M . Calculate how long it takes for the concentration of NH4OH to decrease to 0.0492M . You may assume no other reaction is important. Round your answer to 2 significant digits.
The following enzyme-catalyzed reaction follows zero-order kinetics. When the initial concentration of the reactant is 1.82 M and the rate constant is 0.12 M/min. What will be the remaining concentration in M of the reactant after 4.5 minute? Please report with 2 decimal places, without units. S → P
Using an integrated rate law for a first-order reaction At a certain temperature this reaction follows first-order kinetics with a rate constant of 0.141 s¯¹: H₂CO3(aq) → H₂O (aq) + CO₂ (aq) Suppose a vessel contains H₂CO3 at a concentration of 0.290M. Calculate the concentration of H₂CO3 in the vessel 4.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś