One typical reaction occurring in car engines isNO2+ CO (g)--------> NO (g) + CO2 (g)In order to determine the order of the reaction and the rate constant k, a series of three experiments were performed. The results are shown in the tableExperimentInitial [NO2] (mol/L)Initial [CO] (mol/L)initial rate (v)0.00500.0800.00500.100.400.100.100.100.201231-Write down the general expression for the rate of this reaction2- Find the order for each reactant and the overall order for this reaction. Show your work (3- Find the value for k. Show your work4- Based on these data, do you think that this is an elementary step or not? Briefly explain (

Answered: Image /qna-images/answer/cd475f00-39d9-452f-8fcb-30cc8b784a60.jpg

One typical reaction occurring in car engines is NO2+ CO (g) -------> NO (g) + CO2 (g) In order to determine the order of the reaction and the rate constant k, a series of three experiments were performed. The results are shown in the table Experiment Initial [CO] (mol/L) 0.10 0.10 0.20 Initial [NO2] (mol/L) initial rate (v) 0.0050 0.080 0.0050 0.10 0.40 0.10 1-Write down the general expression for the rate of this reaction 2- Find the order for each reactant and the overall order for this reaction. Show your work( 3- Find the value for k. Show your work 4- Based on these data, do you think that this is an elementary step or not? Briefly explain ( 123

One typical reaction occurring in car engines is NO2+ CO (g) -------> NO (g) + CO2 (g) In order to determine the order of the reaction and the rate constant k, a series of three experiments were performed. The results are shown in the table Experiment Initial [CO] (mol/L) 0.10 0.10 0.20 Initial [NO2] (mol/L) initial rate (v) 0.0050 0.080 0.0050 0.10 0.40 0.10 1-Write down the general expression for the rate of this reaction 2- Find the order for each reactant and the overall order for this reaction. Show your work( 3- Find the value for k. Show your work 4- Based on these data, do you think that this is an elementary step or not? Briefly explain ( 123

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

See image below.
Consider the following reaction and information: A + 2B → 3C rate = k{B} Time (min.) B (M) A (M)0 0.72 0.5030 0.25 0.2660 0.087 0.18 What is the concentration of B after 27 minutes?
How do you determine the overall order of the reaction?
State whether the followingis true or false. If true , explain your reason. if false, explain your reason and provide a correct statement. a) The rate of consumption of reactants and the rate of formation of products is always equal to the rate of reaction (True or false) b) In a reaction A + B ---> P, if the reaction is present in a much higher concentration than reactant A, you can determine the order of reaction with respect to B (True or false) c) In any chemicalreaction A + B ---> C, the concentration of A and B affect the rate of formation of C (True or false)
The following is the experimental data for the rate of reaction: Q (g) + 2T (g) --> T2Q (g) in some conditions Experiment [Q](M) [T](M) V (M/second) 1 0,1 0,1 0,0125 2 0,2 0,1 0,05 3 0,1 0,2 0,1 if [Q] and [T] are changed to 0.5M each, then the reaction rate (v) at that time is?
Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased
A chemistry graduate student is studying the rate of this reaction: H2CO3(ag)>>>H2O(aq)+CO2(aq) She fills a reaction vessel with H2CO3 time (seconds) [H2CO3] 0 0.100M 1.0 0.0259M 2.0 0.0149M 3.0 0.0104M 4.0 0.00803M Use this data to answer the following questions. Write the rate Law for this reaction Calculate the valve of the rate constant A: Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.
Ⓒ Macmillan Learning Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool Add Row 10 total rows [A] [A] vs. t In[A] In[A] vs. t t (min) 0.0 2.0 4.0 6.0 1/[A] vs. t [A] (M) 1.00 0.66 0.43 0.28 1/[A] Clear All Data
Answer Q10, 11, 12
The following initial reaction rates have been measured for the following reaction NO2(g) + O3(g) -> NO3(g) + O2(g) Experiment: Initial Concentration (M) initial rate of the reaction O3 NO2 1 0.7 0.21 6.3 2 1.39 0.21 12.5 3 0.7 0.38 11.4 4 0.18 0.66 X a) Determine the order of and write the rate law of the reaction b) determine the value of K for the reaction. c) Find X
Ln [A] Post Lab Assignment 1. Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl, (g) Determine the rate law, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) Rate (mol L-1 h-1) 0.10 0.20 0.30 3.2 x 10-9 7.2 x 10-9 2. A 5.0 mL dye solution of 3.45 e-5 M is mixed with 15.0 mL bleach solution of 0.21 M. What are the initial concentrations of [Dye] and [Bleach] for your experiment? 3. The plots of 1/[A] vs time, In([A]) vs. time, and [A] vs. time of a solution of substance A are shown below. What is the reaction order with respect to A? 000 009 007 000 0 20 40 Time (min) Time 09 08 Time
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.