Order and rate law of a reactionTo understand how elementary steps make up a mechanism and howthe rate law for an elementary step can be determined.The overall order of an elementary step directly corresponds to its molecularity. Both steps in this example are second order because they are each bimolecular.Furthermore, the rate law can be determined directly from the number of each type of molecule in an elementary step. For example, the rate law for step 1 isVery often, a reaction does not tell us the whole story. For instance,the reactionrate =k[NO2]?NO2(9) + CO(9)¬NO(g)+CO2(g)The exponent "2" is used because the reaction involves two NO2 molecules. The rate law for step 2 isdoes not involve a collision between an NO2 molecule and aCO molecule. Based on experimental data at moderate temperatures,this reaction is thought to occur in the following two steps:rate = k[NO3]"[CO]' = k[NO3][CO]because the reaction involves only one molecule of each reactant the exponents are omitted.1. NO2 (g) + NO2(9)→NO3(9)+NO(g)2. NO3 (9) + CO(9)→CO2(9)+NO2(9)Analyzing a new reactionEach individual step is called an elementary step. Together, theseelementary steps are called the reaction mechanism.Consider the following elementary steps that make up the mechanism of a certain reaction:Overall, the resulting reaction is1. 2X→Y+Z2. Y+ 2L→M+ZNO2 (g) + CO(g)→NO(g)+CO2(g)Notice that in the elementary steps NO3 appears both as a productand then as a reactant; therefore it cancels out of the final chemicalequation. NO3 is called a reaction intermediate. Also notice that 2molecules of NO2 appear in the reactants of the first step and 1molecule of NO2 appears as product of the second step, the neteffect leaves only 1 molecule of NO2 as a reactant in the netequation.Part AWhat is the overall reaction?Express your answer as a chemical equation.• View Available Hint(s)Molecularity is the proper term for "how the molecules collide" in areaction. For example, step 1 is bimolecular because it involves thecollision of two molecules. Step 2 is also bimolecular for the samereason. Unimolecular reactions involve only one molecule in thereactants. Though rare, collisions among three molecules can occur.ΑΣφSuch a reaction would be called termolecular. To understand how elementary steps make up a mechanism and howthe rate law for an elementary step can be determined.Part CVery often, a reaction does not tell us the whole story. For instance,the reactionWhat is the rate law for step 1 of this reaction?NO2 (g) + CO(g)→NO(g)+CO2(g)Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C]³ type k*[A]*[c]^3.does not involve a collision between an NO2 molecule and aCO molecule. Based on experimental data at moderate temperatures,this reaction is thought to occur in the following two steps:• View Available Hint(s)Rate =1. NO2 (g) + NO2(9)→NO3(9)+NO(g)2. NO3 (g) + CO(9)→CO2(g) +NO2 (9)SubmitEach individual step is called an elementary step. Together, theseelementary steps are called the reaction mechanism.Overall, the resulting reaction isPart DNO2(9) + CO(g)→NO(g)+CO2(g)Notice that in the elementary steps NO3 appears both as a productWhat is the rate law for step 2 of this reaction?and then as a reactant; therefore it cancels out of the final chemicalequation. NO3 is called a reaction intermediate. Also notice that 2molecules of NO2 appear in the reactants of the first step and 1molecule of NO2 appears as product of the second step, the neteffect leaves only 1 molecule of NO2 as a reactant in the netequation.Express your answer in standard MasteringChemistry notation. For example, if the rate law is k[A][C]3 type k*[A]*[c]^3.• View Available Hint(s)Rate =Molecularity is the proper term for "how the molecules collide" in areaction. For example, step 1 is bimolecular because it involves thecollision of two molecules. Step 2 is also bimolecular for the samereason. Unimolecular reactions involve only one molecule in thereactants. Though rare, collisions among three molecules can occur.SubmitSuch a reaction would be called termolecular.

The two elementary step give are as follow 1) 2X → Y + Z 2) Y + 2L → M + Z Part A : 1) For…

Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1. 2X→Y+Z 2. Y+ 2L¬M+Z Part A What is the overall reaction? Express your answer as a chemical equation. > View Available Hint(s)

Analyzing a new reaction Consider the following elementary steps that make up the mechanism of a certain reaction: 1. 2X→Y+Z 2. Y+ 2L¬M+Z Part A What is the overall reaction? Express your answer as a chemical equation. > View Available Hint(s)

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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For the chemical reaction NO2(g) + CO(g) → NO(g) + CO2(g) The following initial rate data were obtained Initial [NO₂] Initial [CO] Initial Rate Experiment (mol/L) (mol/L) (mol/L.s) 1 0.10 0.10 0.0050 2 0.40 0.10 0.080 3 0.10 0.20 0.0050 What is the rate law for the reaction? R = k [NO₂]4[CO] R = k [NO₂][CO] R = k [NO₂]²[CO] none of the answers are correct OR = K [NO₂]²
The reaction A -C was performed and the concentration vs. time data below collected. time, s 1 2 3 4 5 6 7 [A], mol/L 0.9088 0.5902 0.3833 0.2489 0.1617 0.1050 0.06818 0.04428 0.02876 Complete the rate law for the reaction by filling in the values for the rate constant and reaction order. Rate = k[A]X rate constant (without units) = reaction order =
initial rate data at a certain temp is given in the table for the reaction (see image) determine the value of the rate constant assuming units of 1/s
3. The kinetics of the following overall reaction was studied: A+B→F +G The following mechanism was suggested: Step 1 (RDS) A + A → A-A Step 2 Step 3 Here is the kinetic data collected: A-A + B → A-B + A A-B → F + G Trial [A] [B] rate (M/s) 1 0.512 0.544 4.06E-4 0.256. 0.544 1.01E-4 3. 0.512 0.333 1.52E-4 FINALLY-the questions! a. Show the rate law for the reaction. b. Is the mechanism shown viable? Explain!
A student studies the concentration of reactant A over time in a reaction and gathers the following data. Use a spreadsheet program (or graph on paper) to determine the order of the reaction with respect to [A] and the rate constant. Enter the numeric value of the rate constant with at least 2 sig figs. time (sec) 0 34.6 82.3 103.1 142.2 179.7 230.0 [A]t [M] 1.146 0.984 0.794 0.708 0.558 0.413 0.233
Using the data in the table, determine the rate constant of the Trial [A] (M) | [B] (M) Rate (M/s) reaction and select the appropriate units. 1 0.220 0.260 0.0189 2 0.220 0.520 0.0189 А + 2B → C+ D 3 0.440 0.260 0.0756 Units 0.0484 k M-'s-1 Incorrect
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Butadiene reacts to form its dimer according to the equation 2C₂H6(8) C3H₁2(8) → The following data were collected for this reaction at a given temperature: [CH] (mol/L) Time (s) 0 120 300 600 1200 1800 2400 3000 3600 0.01000 0.00625 0.00476 0.00370 0.00313 0.00270 0.00241 0.00208 a. Is this reaction first order or second order? b. What is the value of the rate constant for the reaction? c. What is the half-life for the reaction under the conditions of this experiment? Assuming that The decomposition of hydrogen peroxide was studied, and the following data were obtained at a particular temperature: [H₂O₂] (mol/L) Time (±1 s) 0 1000 1800 2800 3600 4400 5200 6200 1.00 0.91 0.78 0.59 0.37 0.22 0.13 0.082 0.050 differential rate law or just Rate = K [H₂O₂]* "rate law". x is order of reaction with respect to H2O2 determine the rate law, the integrated rate law, and the value of the rate constant. Calculate [H₂O₂] at 4000. s after the start of the reaction.
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Mechanism Suppose a reaction occurs with the following mechanism. All are elementary steps. Step 1: 0₂(9) 20(g) fast K₂ Step 2: O(g) + N₂(g) Step 3: O(g) + N(g) گی 3 NO(g) + N(g) slow very fast K3, NO(g) $ 4 % 5 6 What is the rate law for the rate-determining step? Rate =k,[0₂]² Rate = kr[O]² Rate-k,[O][N] Rate = kf[0₂]/k,[0]² Rate = k₂[O][N₂] Rate = K[0₂] & 7 What is the rate law for the forward reaction in step 1? Rate = kr[O]² Rate = kr[0₂] Rate =k+[0₂1² Rate = kr[0₂1² Rate = kf[0]² Rate =k+[0₂] What is the overall rate law for this reaction? Rate = k[N₂][0₂][N][0] MacBook Pro 8 ( 9 ☆ 88
The following initial rate data are for the reaction of ICI with hydrogen: 2IC1 + H₂ → I₂ + 2HCl Experiment [IC]o, M [H₂], M 0.198 0.141 0.396 0.141 0.198 0.281 0.396 0.281 1 2 3 4 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate = k = -2 M-². Initial Rate, M. s-¹ S 0.00657 0.0131 0.0261 0.0522 -1 S