Consider the following mechanisms for the formation of a double helix from its strands A and B: A + B 2 unstable helix (fast) unstable helix → stable double helix (slow) Derive the rate equation for the formation of the double helix and express the rate constant of the reaction in terms of the rate constants of the individual steps. Find the order of the reaction with respect to A and B.

Consider the following mechanisms for the formation of a double helix from its strands A and B: A + B 2 unstable helix (fast) unstable helix → stable double helix (slow) Derive the rate equation for the formation of the double helix and express the rate constant of the reaction in terms of the rate constants of the individual steps. Find the order of the reaction with respect to A and B.

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 overall reaction 2 NO (g) + O2 (g) → 2 NO2 (g) is believed to take place in the following steps: 2 NO (g) N2O2 (g) (fast) N2O2 (g) + O2 (g) → 2 NO2 (g) (slow) Obtain a rate expression that corresponds to this proposed mechanism.
A reaction is found to be second-order with a rate constant of 3.45 × 10–5 M–1 s–1. The reaction initially began with 4.354 M reactant. How much reactant remains (in M to two decimal places) after 1 hour?
For the following second order reaction, the rate constant is 0.0462. If [A]0 = 8.27, calculate [A] at 4.41 seconds. 2 A →→ 3 B
A chemical engineer is studying the rate of this reaction. 2N,0, (g) → 2N,O4g)+O2 (g) He fills a reaction vessel with N,O, and measures its concentration as the reaction proceeds. Here's a graph of his data: 2 1.5 - 0.5 0. 0.2 0.4 0.6 0.8 1.2 t (s) (x) [°o°n]
A chemical engineer is studying the rate of this reaction. 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) She fills a reaction vessel with C1₂05 and measures its concentration as the reaction proceeds. Here's a graph of her data: 2 5 t (s) [C1₂05] (M) 1.5 0.5 0 0
A particular reaction is found to be zero order. The reactant has an initial concentration of 1.52 M and a rate constant of 0.00740 M/s. Calculate the half life of this reactant in seconds. t1/2 =[A]i/2k
What is the rate law for the elementary reaction given below? SO (8) + Cl2 (g) → SOCl2 ()
The following enzyme-catalyzed reaction follows zero-order kinetics. When the initial concentration of the reactant is 1.82 M and the rate constant is 0.12 M/min. What will be the remaining concentration in M of the reactant after 4.5 minute? Please report with 2 decimal places, without units. S → P
The reaction of IC1 with hydrogen 2IC1 + H₂ → I2 + 2HCl is first order in IC1 and third order overall. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate =