The reactionH3C-1 OHH3C-OH+rmay go by either of the following mechanisms:I)H3C-1H3C++r(slow)H3C++ OH ® H3C-OH(fast)orII)H3C-1+ OHH3C-OH+I*If the first mechanism were correct, what would be the rate law?Rate = K[H3C-1]Rate =K[H3C-1][OH]Rate = k[H3C-1][OH-]2Rate =K[H3C][OH]Rate = K[H3C+]

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Answered: The reaction H3C-1 OHH3C-OH+r may go by…

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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One of the reactions that occurs in polluted air in urban areas is 2NO2(g) + O3(g) –→N2O5(g) + O2(g). Assume that a species with the formula NO3 is involved in the mechanism, and the observed rate law for the overall reaction is rate = k[NO2][O3]. Propose a mechanism for this reaction that includes the species NO3 and is consistent with the observed rate law. NO2(g) + O3(g) – NO3(g) + O2(g) (fast) NO3(g) + NO2(g) → N2O5(g) (slow) NO2(g) + O3(g) – NO3(g) + O2(g) (fast) 4NO3(g) 2N2O5(g) + O2(g) (slow) NO2(g) + O3(g) –→ NO3(g) + O2(g) (slow) NO3(g) + NO2(g) → N2O5(g) (fast) NO2(3) + O3(g) → NO3(g) + O2(g) (slow) 4NO3(3) → 2N20O5(g) + O2(g) (fast)
но HO HO HO 0 + ½ O, → + H,0 H H но OH ascorbic acid dehydroascorbic acid Vitamin C is oxidized slowly to dehydroascorbic acid by the oxygen in air. It is catalyzed by ions such as Cu*2 and Fe*3. The reaction can be followed by measuring the ultraviolet absorbance at 243 nm. Time (hours) Absorbance (A) 1/A In A - In A 0.75 1.3 -0.29 0.29 1 0.38 2.6 -0.97 0.97 2 0.19 5.3 - 1.7 1.7 3 0.095 11 - 2.4 2.4 29. What is the hybridization of carbon 1 (far left) and carbon 2 (middle) in this hydrocarbon: CH3CH=CH2? (A) sp³, sp (B) sp?, sp? (C) sp³, sp? (D) sp, sp?
We have the following elementary reactions: A → M + C with the rate constant k1 M + C → A with the rate constant k-1 M + B → P with the rate constant k2 Answer the following questions: 1)Y ou must write down the time derivatives of the concentrations for A, C, M, B and P. This means that you must determine d[X]/dt for all five compounds, where X is one of the compounds A, C, M, B and P. 2) You must show that the reaction rate can be rewritten d [P]/dt = (k1k2)/(k-1[C]+k2[B]) You must assume that you can use the steady state approximation for the concentration of M. 3) You need to examine the expression for the reaction rate: d [P]/dt = (k1k2)/(k-1[C]+k2[B]) for two situations: i) k-1[C]>> k2 [B] ii)k-1 [C]<< k2 [B] and state which elementary reactions are rate-determining in the two situations.
The rate of the reaction N₂O5(g) →2 NO₂(g) + 1/2 0₂(g) is measured at different temperatures, with the following rate constants, k, determined: Temperature, K 298 328 358 378 Recheck k, s-1 1st attempt 3.46 x 10-5 1.5 x 10-3 3.34 x 10-2 0.21 Use the graphing tool above to make an appropriate plot and determine the activation energy, E, for this reaction in units of kilojoules_ X kJ/mol 4 Next) (1 of 1) Show Approach Select functions for the x-axis and the y-axis and create the plot that can be used to find the activation energy. The Arrhenius equatic Ea F/R (1) In k = In A - Inc y=b+mx
Consider the following reaction: 12 (g) + H2 (g) --> 2 HI (g). Given the mechanism below, determine the rate law for the equation. Note: input the rate law following the format rate-k[A]2[B2] with no spaces don't worry about formatting upper or lower case. 1₂ (g) 21 (g) (fast) H₂ (9)+21 (g) → 2HI (g) (slow)
The reaction A + 2 B → C has the rate law rate = k[A][B]. By what factor does the rate of reaction increase when both [A] and [B] are doubled? What is the half-life for a particular reaction if the rate law is rate = (1301 min⁻¹)[A]? Identify the molecularity of the elementary reaction below: 2NO(g) + Br₂(g) → 2NOBr(g) The following reaction is at equilibrium in a closed 4L vessel: N₂(g) + 3H₂(g) ⇌ 2NH₃(g) What will happen if the vessel volume is reduced to 3L? (Assume constant temperature.) If Kc = 82 for the reaction below at 200 K, then what is the value of Kp? 2 NO₂ (g) ⇌ N₂O₄ (g) Consider the reaction: N₂ (g) + 3 Br₂ (g) ⇌ 2 NBr₃ (g) At equilibrium, the concentrations of N₂ and Br₂ are 0.34 M and 0.70 M respectively, and the concentration of NBr₃ is 0.090 M. What is Kc for this equilibrium?
For the following data, determine the rate constant for this reaction: SO2 (g) + Cl2 (g) → SOCl2 + Cl2O (g) Exp [SO2] (M) [Cl2] (M) Rate (M/s) #1 0.400 0.400 0.2918 #2 0.400 0.200 0.0730 #3 0.400 0.800 1.1674 #4 0.200 0.800 0.5837 a). 0.00351 b). 4.56 c). 1.82 d). 9.12
Question 4 Calculate the frequency factor (A). Studies have shown that the reaction occurs via the following mechanism. ki Cl2O4 k-1 Step 1: 2 Cl02 (fast equilibrium) k2 Step 2: C2O4 + OH- → ClO;¯+HCIO2 (slow) k3 Step 3: HCIO2 + OH → ClO2¯+H2O (fast) Question 5: Identify the intermediate/s and the rate-determining step. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 → ClO3¯+HC1O2 Step 2: C204 + OH- (slow) k3 Step 3: HC1O2 + OH- ClO2- + H2O (fast) Question 6 Is the proposed mechanism consistent with the experimentally determined rate law? Show your solution to justify your answer. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 Step 2: C204 + OH- → ClO3¯+ HCIO2 (slow) k3 Step 3: HCIO2 + OH- → ClO2-+ H2O (fast) Question 7 Draw the transition state for Step 3. Identify the bond/s forming/breaking.
The following kinetic data (v, is the initial rate) were ob- tained for the reaction 2 ICI(g) + H,(g) –→ I,(g) + 2 HCI(g): Experiment [ICI]/ V/(mol (mmol dm ) (mmol dm ) dm 3) 1 1.5 1.5 3.7 x 10-7 3.0 1.5 7.4 x 10-7 3 3.0 4.5 22 x 10-7 4 4.7 2.7 ? (a) Write the rate law for the reaction. (b) From the data, de- termine the value of the rate constant. (c) Use the data to predict the reaction rate for Experiment 4.
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Given the following data, determine the rate constant (in M-2s-1) of the reaction 2NO(g) + Cl2(g) –→ 2NOCI(g) [Cl2] (M) Rate (M/s) 3.4 x 104 8.5 x 105 3.4 x 104 Experiment [NO] (M) 1 0.0300 0.0100 0.0150 0.0100 3 0.0150 0.0400 Note: Answers must be numeric, not alphanumeric-42, not forty-two.

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