(1) L(g)=2 I(g)k-(fast, equilibrium)k2(2) I(g) +H,(g) – HI(g) + H(g)(slow)(3) H(g) + I(g)– HI(g)(fast)Which of these mechanisms are consistent with the observed rate law?O mechanism BO mechanism AO mechanism CIn 1967, J. H. Sullivan showed that this reaction was dramatically catalyzed by light when the energy of the light was sufficientto break the I–I bond in an L, molecule. Which mechanism or mechanisms are consistent with both the rate law and thisadditional observation?O mechanism CO mechanism BO mechanism AQuestion Source: McQuarrie, Rock, And Gallogly 4e- General Chemsitry | Publisher:DIIDDF11F10F9888FBF7F5F4&56RT.YHKFM+ CO The reaction described byH, (g) + L,(g) 2 HI(g)has an experimentally determined rate law ofrate = k [H2] [I2]Some proposed mechanisms for this reaction are:Mechanism Ak1(1) H,(g) + L,(g) → 2 HI(g)(one-step reaction)Mechanism Bk1=2 I(g)k_1(1) L(g) ;(fast, equilibrium)k2(2) H, (g) + 2 I(g) 2 HI(g)(slow)Mechanism Ck1= 2 I(g)(fast, equilibrium)(1)k2(2)I(g) + H, (g) HI(g) + H(g)(slow)(3)H(g) + I(g) → HI(g)(fast)Question Sourc

The reaction described by H2 (g) + I2 (g) ---> 2HI(g)

(1) L(g)=21(g) k- (fast, equilibrium) k2 (2) I(g) +H,(g) HI(g) + H(g) (slow) k3 (3) H(g) + I(g): HI(g) (fast) Which of these mechanisms are consistent with the observed rate law? mechanism B mechanism A mechanism C In 1967, J. H. Sullivan showed that this reaction was dramatically catalyzed by light when the energy of the light was sufficient to break the I-I bond in an L, molecule. Which mechanism or mechanisms are consistent with both the rate law and this additional observation? mechanism C mechanism B mechanism A Ouestien Sevrss: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publish

(1) L(g)=21(g) k- (fast, equilibrium) k2 (2) I(g) +H,(g) HI(g) + H(g) (slow) k3 (3) H(g) + I(g): HI(g) (fast) Which of these mechanisms are consistent with the observed rate law? mechanism B mechanism A mechanism C In 1967, J. H. Sullivan showed that this reaction was dramatically catalyzed by light when the energy of the light was sufficient to break the I-I bond in an L, molecule. Which mechanism or mechanisms are consistent with both the rate law and this additional observation? mechanism C mechanism B mechanism A Ouestien Sevrss: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publish

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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2. In the industrial production of hydrogen gas: C,Ha) + 3H,O, - 3CO+ 7H, (), 2(g) The rate molecular hydrogen being produced is 0.098. At what rate is (a) H.O being used? (b) C,H, being consumed? (c) CO being liberated?
Which of the following is TRUE? O In relaxation methods of kinetic analysis, the equilibrium position of a reaction is first shifted suddenly and then allowed to readjust the equilibrium composition characteristi of the new conditions. O Catalysts are substances that accelerate reactions and affect the net chemical change the reaction. O The rate-determining step is the fastest step in a reaction mechanism that controls the rate of the overall reaction O All statements are TRUE O None of the statements are TRUE.
The three-step mechanism outlined in the table below has been proposed for the reaction of chlorine and chloroform. a) Write the equation for the overall reaction. b) Write the rate law for the overall reaction. c) Calculate the rate constant for the overall reaction (include units). elementary steps rate constant (without units) equilibrium constant 1) Cl2(g) <-- --> 2 Cl(g) k1 = 4.8 x 103 Keq1 = 1.2 2) Cl(g) + CHCl3(g) --> HCl(g) + CCl3(g) k2 = 1.3 x 10-2 3) CCl3 + Cl(g) --> CCl4 k3 = 2.7 x 102
Determine if the following proposed mechanisms has a rate law that is consistent with the observed rate law. Reaction: H2+Br2 --> 2 HBr Observed Rate Law for Reaction: rate = k [H2][Br2]1/2 Proposed Mechanism: H2 ⇌ 2 H fast k1 for foward reaction, k1 for reverse reaction H + Br2 --> H Br + Br slow k2 for foward reaction Br + H --> H Br fast k3 for foward reaction
Consider the following reaction mechanism. Step 1: 2X+Y W+ 2 Z fast Step 2: Z U+V slow Step 3: V+Z 2W + Y fast Which of the following is/are the intermediate/s in the given reaction mechanism? O V only O V and Y O Y only O Z and V At 298 K, if the bond dissociation of Cl2g) to Clo) is +57 kJ/mol while the electron affinity of Clg) to form Cl (9) is -349 kJ/mol, then the Gibbs energy of the reaction, Cl2g) + 2e 2 Clg), is negative. Select one: O True O False
The following mechanism has been proposed for the gas- phase reaction of chloroform (CHCI,) and chlorine: Step 1: Cl2(8) 2 CI(g) (fast) Step 2: CI(g) + CHCI3(g) , HCI(8) + CC13(8) (slow) Step 3: CI(g) + CCl;(g) , CC4 (fast) (a) What is the overall reaction? (b) What are the intermedi- ates in the mechanism? (c) What is the molecularity of each of the elementary reactions? (d) What is the rate-determining step? (e) What is the rate law predicted by this mechanism? (Hint: The overall reaction order is not an integer.)
This process may take place in three steps: 2 ClO (g) ⇄ 2 Cl (g) + O2 (g) S1: 2 ClO (g) ⇄ ClOOCl (g)S2: ClOOCl (g) ⇄ ClOO (g) + Cl (g) S3: ClOO (g) ⇄ Cl (g) + O2 (g) Given that rate law for Reaction A is Rate = k[ClO]2, which of the following statements is TRUE? a.) The rate will not change with a change in the concentration of ClO b.) If the concentration of ClO is halved, the reaction rate will be reduced by four c.) If the concentration of ClO is halved, the reaction rate will double d.) If the concentration of ClO is halved, the reaction rate will be reduced in half
R=K [A] [B] ----; 2. The initial rate of the reaction: BrO3(aq) + 5 Br (aq) + 8 H*(aq) Has been measured at the reactant concentrations shown (in mol/L): Trial [BrO3] [Br] [H*] 1 0.10 0.10 0.10 2 0.20 0.10 0.10 3 0.10 0.20 0.10 4 0.10 0.10 0.20 A) Determine the rate law equation including the k value. Determine the order of reaction for BrO3, Br, and H* Rate law 3 Br₂(l) + H₂O(l) Initial rate (mol/Ls) 8.0 x 104 1.6 x 10³ 1.6 x 10°³ 3.2 x 10'³
3) For reaction A ->B All of the following statements for the value of A[A]/ At are true except: a) change as long as the reaction continues. b) The sign is always negative. c) The sign is always positive. d) It depends on the reaction rate law
The following data were obtained for the reaction below at 25.0 °C. 2 NO(g) + O2(g) → 2 NO2(g) Trial 1 2 3 Initial Reactant Concentration (M) [NO] 0.030 0.030 0.060 [0₂] 0.0055 0.0110 0.0055 Initial Rate (M/s) 8.55 x 10-3 1.71 x 10-² 3.42 x 10-² Using the rate law you determined previously, calculate the initial rate for an experiment in which the initial concentration of NO is 0.100 M and O₂ is 0.050 M. Round your answer to 2 sig figs and include your units in your answer.
Write a balanced reaction for which the following rate relationships are true. Rate = - 1 ∆[N2O5] / 2∆t = 1 ∆[NO2] / 4 ∆t = ∆[O2] / ∆t A) 1/2 N2O5 → 1/4 NO2 + O2 B) 4 NO2 + O2 → 2 N2O5 C) 2 N2O5 → 4 NO2 + O2 D) 1/4 NO2 + O2 → 1/2 N2O5 E) 2N2O5 → NO2 + 4 O2