Consider the following reaction mechanism.Step 1:2 X + Y- W + 2 ZfastStep 2:Z- U+ VslowStep 3:V +Z-2 W + YfastWhich of the following is/are the intermediate/s in the given reaction mechanism?O Y onlyO V onlyO Z and VO V and Y

Answered: Image /qna-images/answer/bd6fe513-7873-4b21-9ac7-816650494eac.jpg

Answered: Consider the following reaction…

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter7: Reaction Rates And Chemical Equilibrium

Section: Chapter Questions

Problem 7.58P

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The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution. NH/(aq) + NO2-(aq) — N;(g) + 2 H,O(f) INH/I (mol L1) [NO21 (mol L-1, Rate = A[NJ/At (mol L-1 s’) 0.0092 0.098 3.33 X IO"7 0.0092 0.049 1.66 X 10‘7 0.0488 0.196 3.51 X 10"6 0.0249 0.196 1.80 X 10-6 Determine the rate law for this reaction and calculate the rate constant.
Can a reaction mechanism ever be proven correct? Can it be proven incorrect?
The plot below shows the number of collisions with a particular energy for two different temperatures. a. Which is greater, T2 or T1? How can you tell? b. What does this plot tell us about the temperature of the rate of a chemical reaction? Explain your answer.
The reaction: H2 + I2 = 2HI has an Eactivation = 2000 J/mol. Suppose that it has K=7.5x10-5 M-1s-1 at T=700K, find K at T=800K.
What is the molecularity of the rate limiting step for the mechanism below? Step 1: H2O2 (aq) + I–(aq) → H2O(l) + OI–(aq) (slow)Step 2: H2O2 (aq) + OI–(aq) → H2O(l) + O2 (g) + I–(aq) (fast)
The equilibrium NH3(aq) + H2O(l) ↔NH4+(aq) + OH−(aq) at 25 °C is subjected to a temperature jump which slightly increases the concentration of NH4+(aq) and OH−(aq). The measured relaxation time is 7.61 ns. The equilibrium constant for the system is 1.78 × 10−5 at 25 °C, and the equilibrium concentration of NH3(aq) is 0.15 mol dm−3. (c) Calculate the rate constant for the reverse reaction. krev = _____________. Just value in 3 sig. fig., in normal or exponential format, e.g. 1.16E6 meaning 1.16 x 106 must use capital E. Choose a unit in the next question. .
Rate information was obtained for the following reaction at 25°C and 33°C; Cr(H2O)6 3+ + SCN¯ ---> Cr(H2O)5NCS2+ + H2O(l) Initial Rate [Cr(H2O)6 3+] [SCN-] @ 25°C 2.0x10-11 1.0x10-4 0.10 2.0x10-10 1.0x10-3 0.10 9.0x10-10 2.0x10-3 0.15 2.4x10-9 3.0x10-3 0.20 @ 33°C 1.4x10-10 1.0x10-4 0.20 Can a 4th order reaction occur?
Rate information was obtained for the following reaction at 25°C and 33°C; Cr(H2O)6 3+ + SCN¯ ---> Cr(H2O)5NCS2+ + H2O(l) Initial Rate [Cr(H2O)6 3+] [SCN-] @ 25°C 2.0x10-11 1.0x10-4 0.10 2.0x10-10 1.0x10-3 0.10 9.0x10-10 2.0x10-3 0.15 2.4x10-9 3.0x10-3 0.20 @ 33°C 1.4x10-10 1.0x10-4 0.20 a) Write a rate law consistent with the experimental data. b) What is the value of the rate constant at 25°C? c) What is the value of the rate constant at 33°C? d) What is the activation energy for this reaction? e) Can a 4th order reaction occur?
If Δ[NO]/ Δt = –19.0 M/s under a given set of conditions, what are the rates of change of [N2] and [H2O]?
(a) Can an intermediate appear as a reactant in the firststep of a reaction mechanism? (b) On a reaction energyprofile diagram, is an intermediate represented asa peak or a valley? (c) If a molecule like Cl2 falls apart inan elementary reaction, what is the molecularity of thereaction?
determine the rate constant k of mixture 1, 4, 5 rate = r = k[I-]^1 [S2O82-]^1
Trial [Cl O2] [O H-] Initial rate rxn M/s 1 0.0121 0.25 4.00x10-6 2 0.0242 0.25 2.00x10-6 3 0.0121 0.5 4.00x10-6 4 0.0242 0.75 2.00x10-6 a. Determine the overall order of the reaction if 2 O H- + 2 Cl O2 resulting to products at two hundred ninety eight kelvin b. What is the value of the rate constant? c. What time will it reach in seconds if the chlorine dioxide becomes 1.20 * 10-3 M, starting from 4.00 * 10-3 M

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Consider the following reaction mechanism. Step 1: 2 X + Y- W + 2 Z fast Step 2: Z- U+V slow Step 3: V + Z-2 W + Y fast Which of the following is/are the intermediate/s in the given reaction mechanism? O Y only O V only O Z and V O V and Y