Help on these two plz Analyze a mechanism, including molecularities; write a net reaction; and identify any catalysts or intermediates.A gas phase reaction between nitrogen dioxide and fluorine is proposed to occur by the following mechanism:step 1:NO₂+ F2 NO₂F + FF + NO₂-NO₂Fstep 2:(a) Identify the molecularity of each step in the mechanism.step 1◊step 2C+(b) Write the equation for the net reaction. Use the smallest integer coefficients possible and omit coefficientsof 1. If a box is not needed, leave it blank.+(c) Identify any intemediates and/or catalysts in this mechanism.Close ProblemCatalyst: Enter formula. If none, leave box blank. If coefficient is 1, omit it:Intermediate: Enter formula. If none, leave box blank. If coefficient is 1, omit it: Write the rate law for a mechanism with a slow second step.A kinetic study is done to investigate the following reaction:2 03 3 0₂A proposed mechanism is:Step 1.Step 2.03 20₂ +003 + 0 2 0₂fast in both directionsslow◊(a) Does this mechanism account for the overall reaction?(b) What experimental rate law would be observed if this mechanism is correct?Complete the rate law in the box below.Do not use reaction intermediates and remember that a superscript '1' is not written.Rate =

Answer: Molecularity is related to step of the reaction while order of reaction is the power of…

Analyze a mechanism, including molecularities; write a net reaction; and identify any catalysts or intermediates. A gas phase reaction between nitrogen dioxide and fluorine is proposed to occur by the following mechanism: step 1: NO₂+ F2 NO₂F + F F + NO₂ step 2: (a) Identify the molecularity of each step in the mechanism. step 1 step 2 NO₂F C + 4 (b) Write the equation for the net reaction. Use the smallest integer coefficients possible and omit coefficients of 1. If a box is not needed, leave it blank. Close Problem + (c) Identify any intemediates and/or catalysts in this mechanism.

Analyze a mechanism, including molecularities; write a net reaction; and identify any catalysts or intermediates. A gas phase reaction between nitrogen dioxide and fluorine is proposed to occur by the following mechanism: step 1: NO₂+ F2 NO₂F + F F + NO₂ step 2: (a) Identify the molecularity of each step in the mechanism. step 1 step 2 NO₂F C + 4 (b) Write the equation for the net reaction. Use the smallest integer coefficients possible and omit coefficients of 1. If a box is not needed, leave it blank. Close Problem + (c) Identify any intemediates and/or catalysts in this mechanism.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 3RQ: One experimental procedure that can be used to determine the rate law of a reaction is the method of...

See similar textbooks

Similar questions

One experimental procedure that can be used to determine the rate law of a reaction is the method of initial rates. What data are gathered in the method of initial rates, and how are these data manipulated to determine k and the orders of the species in the rate law? Are the units for k. the rate constant, the same for all rate laws? Explain. If a reaction is first order in A, what happens to the rate if [A] is tripled? If the initial rate for a reaction increases by a factor of 16 when [A] is quadrupled, what is the order of n? If a reaction is third order in A and [A] is doubled, what happens to the initial rate? If a reaction is zero order, what effect does [A] have on the initial rate of a reaction?
The label on a bottle of 3% (by volume) hydrogen peroxide, H2O2, purchased at a grocery store, states that the solution should be stored in a cool, dark place. H2O2decomposes slowly over time, and the rate of decomposition increases with an increase in temperature and in the presence of light. However, the rate of decomposition increases dramatically if a small amount of powdered MnO- is added to the solution. The decomposition products are H2O and O2. MnO2 is not consumed in the reaction. Write the equation for the decomposition of H2O2. What role does MnO2 play? In the chemistry lab, a student substituted a chunk of MnO2 for the powdered compound. The reaction rate was not appreciably increased. WTiat is one possible explanation for this observation? Is MnO2 part of the stoichiometry of the decomposition of H2O2?
For the past 10 years, the unsaturated hydrocarbon 1, 3-butadiene (CH2 = CH - CH = CH2) has ranked 38th among the top 50 industrial Chemicals. It is used primarily for the manufacture of synthetic rubber. An isomer exists also as cyclobutene: The isomerization of cyclobutene to butadiene is first-order and the rate constant has been measured as 2.0104s1 at 150 C in a 0.53-L ?ask. Determine the partial pressure of cyclobutene and its concentration after 30.0 minutes if an isomerization reaction is carried out at 150 C with an initial pressure of 55 torr.
1. Which of the following statements is incorrect? (A) As the chemical reaction proceeds, the rate of reaction increases. (B) The reaction rate almost gets doubled for 10°C rise in temperature. (C) For a first order chemical reaction, the rate constant has unit of time-1. (D) Chemical kinetics can predict the rate of a chemical reaction. 2. In a chemical reaction, represented by A → P, it is observed that the rate of reaction increases by a factor of 4 on doubling the concentration of the reactant. The rate of reaction increases by a factor of 9 on trebling the concentration of the reactant. Then the rate of the reaction is proportional to (A) CA (B) CA2 (C) CA3 (D) CA4 3. An elementary reaction has the stoichiometric equation A + 2B = P. What is the order of reaction (A) 0 (B) 1 (C) 2 (D) 3 4. It states that the rate of a chemical reaction is directly proportional to the product of the activities or concentrations of the reactants. (A) Law of mass action…
rate law for hte reaction : RX + H20→ R0H + HX , rate =K[RX]. the rate of reaction will be doubled when: (a) concentration of H2O is doubled (b)concentration of RX is reduced to half (c) concentration of RX is doubled (d) none of these also give reason for your answer
4. Which of the following statements is incorrect? (A) The rate of a homogeneous reaction is a function of all temperature, pressure and composition. (B) Arrhenius equation shows the variation of rate constant with temperature. (C) Molecularity of a reaction can have a fractional value. (D) If 'n' is the order of reaction, then unit of rate constant is 1/(time)/(concentration)n-1. 5. A molecule have reacted or disappeared when through this method by changing its configuration. (A) Combination(C) Isomerization (B) Decomposition (D) Isolation 6. Rate constant “k” and absolute temperature “T” are related for transition theory as (A) kαTe(-E/RT) (C) kαT2e(-E/RT) (B) kαT0.5e(-E/RT) (D) kαT2.5e(-E/RT) Please answer all!
Be sure to answer all parts. The reaction between NO2 and CO to produce NO and CO2 is thought to occur in two steps: (k1)Step 1: NO2 + NO2 ----> NO + NO3 (k2)Step 2: NO3 + CO ---->NO2 + CO2 The experimental rate law is rate = k[NO2]2. (a) Write the equation for the overall reaction. Do not include phase abbreviations. (b) Identify the intermediate(s). (c) Identify the rate-determining step.
(a) Select all of the correct statements about reaction rates from the choices below. The lower the rate of a reaction the longer it takes to reach completion.Reactions involving very unstable combinations of chemicals have large rate constants.Concentrations of homogeneous catalysts have no effect on reaction rates.Reaction rate constants are independent of temperature.The slowest step in a reaction is called the rate-determining step.A balanced chemical reaction is necessary to relate the rate of reaction to the concentration of a reactant.Slow reactions can be speeded up by raising the temperature.
Consider the following Potential Energy Diagram for a four-step reaction mechanism. (a) What is the overall balanced equation for the reaction? (b) Does this reaction have a catalyst? Explain how you know. (c) Which step in the above mechanism is the rate-determining step? (d) Is this reaction exothermic or endothermic? (e) The rate law equation was determined to be rate = k [NO2] [F2]. Is the proposed mechanism plausible?
1 The gas phase reaction of chloroform is described by the following equation, experimental rate law and proposed mechanism. (a.) Does this proposed mechanism agree with the overall reaction? (b.) What intermediates are present in this reaction? (c.) Does the experimental rate law agree with the mechanism provided? (d.) Write the overall reaction rate constant in terms of the rate constants of the elementary steps. NOTE: The rate law should have Cl2 not Cl in the brackets. The experimental rate law will be k[C12]^(1/2)[CHC13]. Please make this correction. (Non-anonymous questionO) (20 Points) %3D Overall Reaction: Cl2(g) + CHCI3(g) → HCI(g) + CCl4(g) Experimental Rate Law = k[CI]!/2[CHCI3] Proposed Mechanism: 1. Cl2(g) E→ 2CI(g) 2. Cl(g) + CHCI3(g) → HCI(g) + CCI3(g) 3. Cl3(g) + Cl(g) →CCI«(g) fast slow fast
(a) What is the reaction order of the reactant H2 in Equation14.10? (b) What are the units of the rate constant forEquation 14.10? H2(g) + I2(g)------>2 HI(g) Rate = k[H2][I2] [14.10]
3. (2) What are the units of k in the following rate law if rate is measured in sec-¹? Rate = K[X]³[Y]³ 4. (4) The isomerization of cyclopropane to propene follows first-order kinetics. H₂C -CH₂ H₂C-CH=CH₂ CH₂ At 700 K, the rate constant for this reaction is 6.2 x 104 min¹. How many minutes are required for 10.0% of a sample of cyclopropane to isomerize to propene? -