step elementary reaction rate constant 1 NO₂(g) + F₂(g) → NO₂F(g) + F(g) k₁ 2 F (g) + NO₂(g) - NO₂F (g) k₂ Suppose also k₁k2. 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. k = U 0-0 믐 010 X C

step elementary reaction rate constant 1 NO₂(g) + F₂(g) → NO₂F(g) + F(g) k₁ 2 F (g) + NO₂(g) - NO₂F (g) k₂ Suppose also k₁k2. 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. k = U 0-0 믐 010 X C

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

Similar questions

The reaction between N2O5 and water$$N2O5(g)+H2O(g)2HNO3(g)is a source of nitric acid in the atmosphere. The reaction is first order in each reactant. Write the rate law for the reaction.
Chlorine oxide (CIO), which plays an important role in the depletion of ozone, decays rapidly according to the equation 2CIO(g) →→→ Cl₂(g) + O₂(g) - From the following data, determine the reaction order and calculate the rate constant of the reaction. Time (s) [CIO] (M) 2.91 x 103 8.11 × 10-6 3.64 x 10-3 5.77 × 10-6 4.37x103 4.48 x 10-6 5.10 x 10 3 3.66 x 10-6 5.83 x 10-3 3.09 x 10-6 Reaction order: O O 1 2 Rate constant: k = x 10 Ms (Enter your answer in scientific notation.)
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
10. The reaction 2NO+2H₂ →→→ N₂ + 2H₂O is proposed to occur through the following two elementary steps: k₂ H₂(g) + 2NO(g)- N₂O(g) + H₂O(g) H₂(g) + N₂O(g) N₂(g) + H₂O(g) By using the steady state approximation, what would be its rate expression? A) R = K[H₂][NO]2 B) R= K[H₂][NO] C) R = K1 K2 [H₂][NO]2 D) R=(k/k₂) [H₂][NO]2 E) R = K[H₂]2[NO]² *
The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]
The hydrolysis of the sugar sucrose to the sugars glucose and fructose can be described as follows. C12H22O11 + H2O → C6H12O6 + C6H12O6 This reaction follows a first-order rate equation for the disappearance of sucrose: rate = k [C12H22O11] (The products of the reaction, glucose, and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules, i.e. they are isomers.) (a) In neutral solution, k = 1.8 ✕ 10−11 s−1 at 26°C and 8.5 ✕ 10−11 s−1 at 37°C. Determine the activation energy (in kJ/mol), the frequency factor (in s−1), and the rate constant (in s−1) for this equation at 48°C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (Enter unrounded values.) FREQUENCY FACTOR??_________ RATE CONSTANT?? _________ (b) When a solution of sucrose with an initial concentration of 0.130 M reaches equilibrium, the concentration of sucrose is 1.40 ✕ 10−7 M. How long (in s) will it take the…
Questions 2A 2B and 2C please
You are studying the reaction A₂(g)+B₂(g) →2AB(g) to determine its rate law. Assuming that you have a valid exper-imental procedure for obtaining [A₂] and [B₂] at various times,explain how you determine (a) the initial rate, (b) the reaction orders, and (c) the rate constant.
Please complete the question typed ONLY. Please do not use handwriting.
4
The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism: 2 NO(g) --> N2O2(g)N2O2(g) + O2(g) --> 2 NO2(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [O2] Rate = k [NO] [O2]1/2 Rate = k [NO]2 Rate = k [NO]2 [O2]1/2 Rate = k [NO]
The observed rate law for the reaction 20₂(g) →30₂(g) is Rate = k[O3]²/[0₂]. Is it improbable that the reaction occurs in one step: O₂(g) + O₂(g) → O₂(g) + O₂(g) + O₂(8) ? Why or why not?