= constant is k, when the ionic strength (I) is 0.004. And the rate constant is k when the activity coefficient is 1. The ration k /k 2 = 0.884. If the charge of one ion is +1, the charge of other ion is close to (Debye-Hückel constant - 0.509 at 298K; log 0.884 = - 0.05) दो आयनों के मध्य की अभिक्रिया में, जब आयनी सामर्थ्य (I) 0.004 है, वेग नियतांक k है। तथा जब सक्रियता गुणांक 1 है, तब वेग नियतांक k है। अनुपात _k/k 2 = 0.884 है। यदि एक आयनं का आवेश + 1 है, तब दूसरे आयन का आवेश जिसके निकटतम है, वह है • (298 K पर डिबाई-हुकल (Hickel) नियतांक 11 0.509; log 0.884 = - 0.05) (a) - 1.554 (b) -1.395 (c) -0.777 (d) – 0.389

= constant is k, when the ionic strength (I) is 0.004. And the rate constant is k when the activity coefficient is 1. The ration k /k 2 = 0.884. If the charge of one ion is +1, the charge of other ion is close to (Debye-Hückel constant - 0.509 at 298K; log 0.884 = - 0.05) दो आयनों के मध्य की अभिक्रिया में, जब आयनी सामर्थ्य (I) 0.004 है, वेग नियतांक k है। तथा जब सक्रियता गुणांक 1 है, तब वेग नियतांक k है। अनुपात _k/k 2 = 0.884 है। यदि एक आयनं का आवेश + 1 है, तब दूसरे आयन का आवेश जिसके निकटतम है, वह है • (298 K पर डिबाई-हुकल (Hickel) नियतांक 11 0.509; log 0.884 = - 0.05) (a) - 1.554 (b) -1.395 (c) -0.777 (d) – 0.389

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 53AP

See similar textbooks

Similar questions

If the slope is 0.0100 for this reaction, determine the rate constant, k, for this reaction.
The recombination reaction2 HO2(g) → H2O2(g) + O2(g)has a second-order rate constant of 1.7E9 M-1 s-1. Calculate the half-life of the reaction if the initial concentration of HO2(g) is 2.22E-11 M.Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is:1/ct = 1/c0 + 2kt Give the answer to 3 significant figures
what is the form of the integrated rate law which will produce a straight line if the following reaction that we observing dye(aq) + NaOCL(aq) --> colorless product (aq) is second order with respect to dye?
Two kinetics trials are performed at the same temperature with [S2O82-] held constant. The first trial has a reaction time of 84 seconds. For the second trial, the [I ̶ ] is four times that of the first trial (the concentration is quadrupled), and the reaction time is 22 seconds. If the change in concentration of S2O82- is 4.3x10 ̶ 5 M for both trials, what is the reaction order with respect to iodide ion?
The recombination reaction2 HO2(g) → H2O2(g) + O2(g)has a second-order rate constant of 2E9 M-1 s-1. Calculate the half-life of the reaction if the initial concentration of HO2(g) is 2.58E-11 M.Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is:1/ct = 1/c0 + 2kt
The reaction rate units for order 3 kinetics. Are they L2/mol2·s or L2/mol/s?
1. What is the difference between the Freundlich and Langmuir isotherm models in adsorption? 2. What is the difference between Pseudo-First Order and Pseudo-Second Order of kinetics?
Many metallic catalysts, particularly the precious-metalones, are often deposited as very thin films on a substanceof high surface area per unit mass, such as alumina(Al2O3) or silica (SiO2). (a) Why is this an effective way ofutilizing the catalyst material compared to having powderedmetals? (b) How does the surface area affect the rateof reaction?
A reaction was observed to have a first dependence to AB and second order dependence to C2. What is the reaction's rate law?
Below is a proposed mechanism for ClO–(aq) reacting with I–(aq) in the presence of OH–(aq). ClO- +H2O --> HOCl +OH- (fast, reversible)I- +HOCl --> HOI +Cl- (slow)HOI + HO- --> IO- +H2O You are trying to show that the rate law for this proposed mechanism matches an experimentallydetermined one. What is the expression for koverall or k’ for the proposed mechanism?Note: When writing an expression, H2O is not involved (just don’t include it).
The Haber process, also called the Haber–Bosch process, is an artificial nitrogen fixation process and is the main industrial procedure to produce ammonia today. In agriculture, ammonia is produced with the help of iron catalysts. The ammonia is most used in the field to make fertilizers which are essential for plant growth. What type of catalytic mechanism (heterogenous or homogenous) is involved in Haber’s or Bosch process in producing ammonia? Explain why? Why activation energy is important to start a chemical reaction? What is the relationship between catalyst and activation energy? How do you call the catalyst that slows down chemical reaction?
Why may some gas-phase reactions show fi rst-order kinetics?