1The gas phase reaction of chloroform is described by the following equation, experimentalrate 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 elementarysteps.NOTE: The rate law should have Cl2 not Cl in the brackets. The experimental rate law will bek[C12]^(1/2)[CHC13]. Please make this correction. (Non-anonymous questionO)(20 Points)%3DOverall 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)fastslowfast

Here we have to determine the overall reaction from the mechanism of reactions, intermediate in…

Overall Reaction: Cl2(g) + CHCI3(g) → HCI(g) + CCl«(g) Experimental Rate Law = k[CI]!/2[CHCI3] Proposed Mechanism: 1. C2(g) E→ 2CI(g) 2. Cl(g) + CHCI3(g) → HCI(g) + CCI3(g) 3. Cla(g) + Cl(g) →Cla(g) fast slow fast

Overall Reaction: Cl2(g) + CHCI3(g) → HCI(g) + CCl«(g) Experimental Rate Law = k[CI]!/2[CHCI3] Proposed Mechanism: 1. C2(g) E→ 2CI(g) 2. Cl(g) + CHCI3(g) → HCI(g) + CCI3(g) 3. Cla(g) + Cl(g) →Cla(g) fast slow fast

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

Related questions

Q: You perform some experiments for the reaction A → B+C and determine the rate law has the form Rate =…

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: Avalid mechanism for the following overall reaction is given below. Overall reaction: 2 NO (g) + Cl2…

A: The rate law for the mechanism of the overall reaction can be obtained from the slowest step…

Q: Consider the following chemical equation: Overall Reaction: 2AB +2C2 - A2 + 2C,B The proposed…

A: Rate law : Rate law is the expression which gives rate of reaction interms of molar concentration…

Q: The reaction CHCl3(g) + Cl₂(g) → CCl4(g) + HCI(g) is believed to proceed by this mechanism: Cl₂(g)…

A: Rate of reaction is given by the slowest step of the mechanism.The rate of reaction must not include…

Q: Consider the proposed mechanism for the reaction, CHCl3(g) + Cl2(g) --> HCl(g) + CCl4(g)…

A: Consider the proposed mechanism for the reaction, A student proposes that the reaction rate law…

Q: Nitryl bromide, NO2Br, decomposes into nitrogen dioxide and bromine. 2NO2Br(g) → 2NO2(g) + Br2(g)…

Q: Consider the following three-step mechanism for a reaction: Cl2 (g) = 2 CI (g) Fast CI (g) + CHCI3…

A: The rate law of the reaction is given by,

Q: Find the rate law for the reaction 2 N205(g) – 4 NO2(g) + O2(g) based on the proposed mechanism: NO2…

A: The rate of the overall reaction depends on the rate of the slow step only. Therefore, the rate law…

Q: The proposed mechanism for the formation of hydrogen bromide can be written in a simplified form as:…

A: The reaction of hydrogen bromide formation is a multistep process. This process is consist of 3…

Q: (b) What is the value of the rate constant? 8.67e-3 ✔ M²5-1 (c) What is the reaction rate when the…

Q: Even when a mechanism is consistent with the rate law,later work may show it to be incorrect. For…

A: Given: The overall reaction is as follows, The rate of reaction is as follows,

Q: H2 (g) + 2 ICl (g) → I2 (g) + 2 HCl (g) The observed rate law is Rate = k [H2][ICl]. A proposed…

A: The given reaction is, H2 (g) + 2 ICl (g) → I2 (g) + 2 HCl (g) Rate law is, Rate = k [H2][ICl]…

Q: The reaction 2 H2 (g) + 2 NO (g) → N2 (g) + 2 H20 (g) is proposed to occur via the following…

A: Answer :- d) rate = k[H2][NO] -----------------------------------------------------

Q: ch rate law

Q: The rate for the overall reaction NO2 (g) + CO (g) → NO (g) + CO2 (g) is Rate = k[NO2]2 a.…

A: Since you have asked a question with multiple sub-parts, we will solve first three sub-parts for…

Q: The rate for the overall reaction NO2 (g) + CO (g) ® NO (g) + CO2 (g) is Rate =…

Q: In a study of nitrosyl halides, a chemist proposes the fol-lowing mechanism for the synthesis of…

A: The rate law relates the rate constant and concentration of reactants and products taking part in…

Q: The mechanism for the reaction described by NO2(g)+CO(g)⟶CO2(g)+NO(g) is suggested to be…

A: In this equation, we want to drive rate law expression by using given mechanism. . I will give…

Q: What is the molecularity of the rate-determining step in the proposed mechanism? Step 1 Step 2 H₂(g)…

A: Rate-determining step : It is the slowest step of a multi-step chemical reaction that determines the…

Q: Consider the following three-step mechanism for a reaction: Step 1: Cl2(g)2Cl(g), fast Step2:…

A: Rate law is the product of concentrations of the reactents

Q: Iodide ion is oxidized by hydrogen peroxide in acidic solution. H2O2 (aq) + 31 (aq) + 2H† (aq) → I5…

A: Given reaction: H2O2 (aq) + 3I- (aq) +2H+ (aq) → I3- (aq) + 2H2O (l) Given rate law of the reaction:…

Q: The following reaction 2 NO(g) + O₂(g) → 2 NO₂(g) was found to be first order in each of the two…

A: In rate equation the sum of the powers of concentration terms indicates the order of the reaction.…

Q: For reaction 2A2(g) + B2(g) ⟶ 2A2B (g), the reaction is 1st order with respect to A2 and 2nd order…

Q: 6. The rate law for the overall reaction 2 N2O5 (g) →4 NO2 (g) + O2 (g) is Rate = k[N2Os). a.…

A: a) When a proposed mechanism consists of more than one elementary step, the one with the slowest…

Q: 1a) CO(g) + Cl2(g) COCl2(g) The above reaction obeys the mechanism: Cl2 2Cl Fast equilibrium…

A: Given:-

Q: For the following reaction: H2(g) + ICl(g) ----> HI(g) + HCl(g) slow HI(g) + ICl(g) ---> I2(g) +…

A: Rate law equation

Q: Given the initial rate data below, what is the rate law for the reaction? CO (g) + NO2 (g) CO2 (g) +…

A: COg + NO2g --> CO2g + NOg LET Rate= k × COgA × NO2gBWhere A = Order with…

Q: the following reaction 2 NO(g) + O2(g) --> 2 NO2(g) was found to be first order in each of the two…

A: The relation between the concentration of the reactants and the rate of reaction is expressed by the…

Q: Consider the reaction described by the equation C2H4Br2(aq)+3I−(aq)⟶C2H4(g)+2Br−(aq)+I−3(aq) The…

A: Given: Rate constant = 0.00409 M-1s-1. And the rate law of the reaction = K [C2H4Br2] [I- ]

Q: Be sure to answer all parts. The reaction of peroxydisulfate ion (S2O82−) with iodide ion (I−) is…

A: The reaction of peroxydisulfate ion (S2O82−) with iodide ion (I−) is S2O82−(aq) + 3I−(aq) →…

Q: The reaction H2(g) + I2(g) → 2HI(g) may occur by the mechanism shown above. What is the rate law…

A: The relation between the concentration of the reactants and the rate of reaction is expressed by the…

Q: ¹₂(g) + ICl(g) → HI(g) + HCl(g) HI(g)+ ICI(g) 1₂(g) + HCl(g) Suppose also k₁«k₂. That is, the first…

Q: Given the following proposed mechanism, predict the rate law for the overall reaction. 2NO2 + Cl2 →…

A: If the reaction goes via more than one step then the rate depends on the slowest step of the…

Q: Consider the following reaction mechanism for the addition of HCl to propene in the gas hase. The…

A: As given that the third step is the rate determining step, so rate law is given as: Rate =…

Q: The reaction of NO gas with H2 gas has the following rate law: Rate = k[H2][NO]2. A proposed…

A: Since we can see that in reaction step 1 we habe 1 H2 and 2 NO molecules reacting And since…

Q: 6. The rate law for the overall reaction 2 N2O5 (g) →4 NO2 (g) + O2 (g) is Rate = k[N2O5]. a.…

A: “Since you have posted a question with multiple sub-parts, we will solve the first three subparts…

Q: Consider the proposed mechanism for the reaction, CHCI3(g) + Cl2(g) HCI(g) + CCI4(g) --> (1 - fast)…

A: Given mechanism is : Overall reaction is :

Q: The overall reaction 2 NO (g) + 02 (g) → 2 NO2 (g) is believed to take place in the following steps:…

Q: is the missing initial rate (marked with a "?" in the

A: From the experimental data, Rate = k[H2]C2H4] So,order with respect to H2 and C2H4 is 1. From…

Q: 2 NO (g) + O₂ (g) --> 2 NO2 (g) The proposed mechanism for the reaction above is 1) NO (g) + NO (g)…

A: Answer: For a multistep reaction, slowest step is always the rate determining and since, over here…

Q: 8. For the overall reaction: 2NO (g) +O2 (g) → 2NO2 (g), the following mechanism has been proposed:…

Q: One of the reactions that occurs in polluted air in urban areas is 2NO2(g) + O3(g) –→N2O5(g) +…

A: The net reaction : 2NO2(g) + O3(g) ---> N2O5(g) + O2(g) rate = k [NO2] [O3] Mechanism for the…

Q: The rate for the overall reaction NO2 (g) + CO (g) → NO (g) + CO2 (g) is Rate = k[NO2]². a.…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: For the reaction 3O2(g) + 4NO(g) → 2N2O5(g) the rate of change in concentration of O2, Δ[O2]/Δ t =…

A: Answer:To relate the rate of change in concentration of reactant and product divide their respective…

Question

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

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Overall Reaction: 2AB + B2 → 2AB2 The proposed mechanism is as follows: AB + B2 ⇋ AB3 (fast) AB3 + AB → 2AB2 (slow) What is the rate law?
Suppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant 1 03(g) O₂(g) + 0(g) k₁ 2 03(g) + O(g) → 20₂(g) k₂ Suppose also k₁ »k₂. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally- observable rate law for the overall chemical reaction. rate = k Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of K₁, K2, and (if necessary) the rate constants k.1 and k-2 for the reverse of the two elementary reactions in the mechanism. = 0 k = 00 X 5 S ?
10 2NO₂Cl(g)2NO₂(g) + Cl₂(g) The following mechanism is proposed: NO₂Cl(g) NO₂(g) + Cl(g) NO₂Cl(g) + Cl(g) → NO₂(g) + Cl₂(g) slow Which of the following rate laws is consistent with this mechanism? rate= K[NO₂CI]2[NO2]-1 rate = K[NO₂CI]²[NO2] rate = K[NO₂CI] rate=k[NO₂CI]² rate=k[NO₂][NO₂CI] X (no answer) Correct Answer: rate= K[NO₂CI]²[NO2] 1 fast equilibrium
Serial No. - Consider the reaction: 2 NO(g) + Cl₂(g) -2 NOCI(g) 2 Derive a rate law for the reaction based on the following mechanism: NO(g) + Cl₂ → NOCI(g) + CI(g) NO(g) +CI(g) NOCI(g) (1) fast slow
For the reaction mechanism shown, identify the intermediate(s). Cl2(g) = 2CI(g) CHCI3(g) + CI(g) = HCI(g) + CCl:(g) CCI3(g) + CI(g) = CCI4(g)
4.) The overall reaction 2NO2(g) + F2(g) →2NO2F(g) has an experimental rate law Rate = k[NO2][F2]. The accepted two step mechanism is: %3D (1) NO2(g) + F2(g) → NO2F(g) + F(g) (2) NO2(g) + F(g) → NO,F(g) [slow; rate determining] [fast] a. Write the rate laws for each of the elementary steps. b. What is the molecularity for each step? C. Show how the elementary steps sum to the overall balanced equation: d. Which species (if any) are intermediates? Which step is rate-limiting? e. f. Is the mechanism reasonable and consistent with the observed rate law? Explain
The rate for the overall reaction NO2 (g) + CO (g) → NO (g) + CO2 (g) is Rate = k[NO2]2 a. Consider this mechanism: i. 2NO2 (g) → N2 (g) + 2O2 (g) [slow] ii. 2CO (g) + O2 (g) → 2CO2 (g) [fast] iii. N2 (g) + O2 (g) →2NO (g) [fast] d. Draw a reaction energy diagram for this mechanism, given that the overall reaction’s ΔH°rxn = -226 kJ/mol.
What is the rate law of the reaction NO2(g) + CO(g) ó NO(g) + CO2(g) If the mechanism behind it is : 2NO2(g) à 2NO(g) + O2(g) (slow) NO(g) + CO(g) + O2(g) à NO2(g) + CO2(g) (fast) Rate of reaction is rate of slow step. Rate = k [NO2]2
Suggest a mechanism behind the reaction NO(g) + Cl2(g) à NOCl(g) + Cl(g) with the rate law rate = k [NO]2 [Cl2] This reaction cannot be a one step reaction because of its rate law. It is therefore a multistep reaction, where the slow step represents a reaction between 2 molecules of NO with one molecule of Cl2 (slow) 2NO + Cl2 à ………. (fast). à ………… NO + Cl2. à NOCl + Cl
A valid mechanism for the following overall reaction is given below. Overall reaction: 2 NO (g) + Cl2 (g) → 2 NOCI (g) Step 1: NO (g) + Cl2 (g) → NOCI2 (g) Step 2: NOC12 (g) + NO (g) → 2 NOCI (g) (slow) (fast) What is the rate law for this reaction? Rate = k[NO]?[Cl2] Rate = k[NO][CI] Rate = k[NO][Cl2][NOCI] Rate = k[Cl2][NOC12]
4) A possible mechanism for the overall reaction Br2 (g) + 2NO (g) → 2NOBr (g) is NO (g) + Br2 (g) NOBr2 (g) (fast) NOBr2 (g) + NO (g) 2NOBr (slow) The rate law for formation of NOBr based on this mechanism is rate = ________. a. k1[NO]1/2 b. k1[Br2]1/2 c. (k2k1/k-1)[NO]2[Br2] d. (k1/k-1)2[NO]2 e. (k2k1/k-1)[NO][Br2]2
The mechanism for the reaction described by NO₂(g) + CO(g) → CO₂(g) + NO(g) is suggested to be k₁ (1) 2 NO₂(g) NO₂(g) + NO(g) k₂ (2) NO3(g) + CO(g) → NO₂(g) + CO₂(g) Assuming that [NO] is governed by steady-state conditions, derive the rate law for the production of CO₂ (g). rate of CO₂ (g) production =