Question 2 W Step 1: H2(g) + IC1(9) → HI(g) + HCl(9) (slow) Step 2: HI(g) + ICI(g) → HCl(g) + I2(g) (fast) Which of the following represents a rate law for the overall reaction that is consistent with the proposed mechanism? A Rate = k[H2] [ICI] %3D Rate = k [H2] [ICI]² B Rate = k[H2] [HI] [IC1]² Rate = k[HI] [ICI] D %3D

Question 2 W Step 1: H2(g) + IC1(9) → HI(g) + HCl(9) (slow) Step 2: HI(g) + ICI(g) → HCl(g) + I2(g) (fast) Which of the following represents a rate law for the overall reaction that is consistent with the proposed mechanism? A Rate = k[H2] [ICI] %3D Rate = k [H2] [ICI]² B Rate = k[H2] [HI] [IC1]² Rate = k[HI] [ICI] D %3D

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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Answer all parts
Question 1 Consider the reaction mechanism for NO2(g) + CO(g) → CO2(g) + NO(g) (1) NO₂(g) + NO₂ (g) → NO3(g) + NO (g) (slow) (2) NO3(g) + CO (g) → CO₂(g) + NO₂(g) - Write the letter of the correct answer. 1. Which is the rate-determining step? 2. Which is the fast step? A. Step 1 B. Step 2 3. Which is the intermediate? 4. Which is the catalyst? A. CO B. NO C. NO2 D. NO3 E. CO2
2
Nitrous oxide, NO, reacts with hydrogen to produce nitrogen and water. The initial rate data obtained for this reaction are given below: NO(g) + H2(g) –→ N2(g) + H2O(l) Using this data, determine the experimental rate law and calculate the rate constant. Experiment [NO] / mol L-1 [H2] / mol L-1 Initial Rate / mol L-1 s-1 1 0.420 0.122 0.136 0.210 0.122 0.0339 3 0.210 0.244 0.0678
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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
physical chemistry
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