Write the overall reaction and the rate laws that corre- spond to the following reaction mechanisms. Be sure to eliminate intermediates from the answers. (a) 2 A + B = D (fast equilibrium) k-s k2 D + B → E + F (slow) ks F , G (fast) (b) A + B= C (fast equilibrium) k2 C+D 2 F k-2 (fast equilibrium) k F , G (slow)

Write the overall reaction and the rate laws that corre- spond to the following reaction mechanisms. Be sure to eliminate intermediates from the answers. (a) 2 A + B = D (fast equilibrium) k-s k2 D + B → E + F (slow) ks F , G (fast) (b) A + B= C (fast equilibrium) k2 C+D 2 F k-2 (fast equilibrium) k F , G (slow)

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

What is the order with respect to reactant G? G+J Product |GJ M 0.10 [J] M Initial Rate (M-s-') 2.2x104 0.15 0.20 0.15 8.8x104 4.4x104 0.10 0.30 (A) 4 (B) 2 (C) 1 (D) 0
Be sure to answer all parts. For the following general reaction, rate = k[A]2 and k=1.3 × 10 2 M¹g¹; A+B 2C Use this information to fill in the missing table entries. Experiment [A] (M) [B] (M) Initial rate (M/s) 1 0.013 0.250 2.20 × 10-6 2 0.026 0.250 3 0.500 2.20 × 10-6 1) Initial reaction rate in experiment 2: x 10 M/s (Enter your answer in scientific notation.) 2) Initial concentration of A in experiment 3: M
= ◇ KINETICS AND EQUILIBRIUM Expressing the concentration of an intermediate in terms of the... Consider the following elementary reaction: 2 NO₂(g) → NO₂(g) + NO(g) Suppose we let k₁ stand for the rate constant of this reaction, and k_₁ stand for the rate constant of the reverse reaction. Write an expression that gives the equilibrium concentration of NO₂ in terms of k₁, k₁, and the equilibrium concentrations of NO and NO. [NO₂] = 0 X 2 8 1/5
What is the concentration of A after 37.5 minutes for the reaction A → Products when the initial concentration of A is 0.750 M? (k = 0.0451 M⁻¹min⁻¹)
Please use the following information to answer the next 3 questions: Step 1: Step 2: Step 3: A + B → C C + D E + 2 M D + E + B J 14. Identify all intermediates. eחסח A and E only Conly C, D and E only C and E only 15. Identify the catalysts. C, D and E only C only none A and E only C and E only 16. Identify the products in the overall reaction. C, E and M only M and J only M and E only Jonly C, E, M and J
Hi i am having trouble with this portion of the question. Please provide handwritten solution for better understanding CO(g) + Cl2(g) COCl2(g) The above reaction obeys the mechanism: Cl2 --> 2Cl Fast equilibrium Cl + CO--> COCl Fast equilibrium COCl + Cl2 --> COCl2 + Cl Slow 2Cl--> Cl2 Fast 1b) Suppose that: k1/k-1 = 1×10-2 mol L-1, k2/k-2 = 1×106 L mol-1, k3 = 1×10-4 L mol-1 s-1, and k4 = 1×103 L mol-1 s-1. What would be the value of the overall rate constant, k, including the correct units?
For the reaction X + 5Y + 6Z --> 3A + 4B at a particular time, -A[X]/At = 1.5x10-2 M/s. What is A[A]/At at the same instant?
What is the relationship between the equilibrium constant, the concentration of each component of the system, and the rate constants for the forward and reverse reactions? [A]" [B]b _ kr For a A+BBCC +d D, K = cjDja = kr For a A+b B cC+d D, K =- [C[D]d _ kg [A][B]b k, [C](D]d kr [A] [B]b kr For a A+b B c C+d D, K =: %3D For a A+bBcC+d D, K = AB= k !3! [C[D]d k,
What is the concentration of A after 30.5 minutes for the reaction A → Products when the initial concentration of A is 0.750 M? (k = 0.0451 M⁻¹min⁻¹)
Using the following reaction: A + 2B → C + D Describe how the rate of disappearance of B will compare to the rate of appearance of C at the start of a reaction. It is determined that A and B are first order reactants. Explain how you would write out the rate law and units of the equilibrium constant with respect to the equation above.
For a decomposition reaction, the values of k at two different temperatures are given below:k1 = 2.15 × 10-8 L mol-1 s-1 at 650 Kk2 = 2.39 × 10-7 L mol-1 s-1 at 700 KCalculate the value of activation energy for this reaction.(Log 11.11 = 1.046) (R = 8.314 J K-1 mol-1)
If a catalyst is added, what direction would the equilibrium position shift to?