The reduction of peroxydisulfate ion (S₂02) by iodide ions to form sulfate ions and aqueous iodine is very slow unless iron(II) or iron(III) ions are present. The iron ions are a contaminent. a heterogeneous catalyst. an inhibitor. O a homogeneous catalyst.

The reduction of peroxydisulfate ion (S₂02) by iodide ions to form sulfate ions and aqueous iodine is very slow unless iron(II) or iron(III) ions are present. The iron ions are a contaminent. a heterogeneous catalyst. an inhibitor. O a homogeneous catalyst.

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

Determine the rate law and the value of k for the following reaction using the data provided. NO,(9) + O3(g) – NO3(g) + O2(g) [NO,li (M) 0.1 0.1 [03li (M) Initial Rate (ms-1) 1 0.33 1.42 2 0.66 2.84 0.25 0.66 7.10 Rate = 43 M's INO,0,] S. -25c O Rate = 1360 M2s"INO,110,] S. Rate = 227 M25s INO,J[0,125 O Rate = 430 M?s INO,10,
8. Using the correct catalysts and solvents, what are the likely product outcomes of steps I and III of the following reaction? 1. PBr3 2. Br2 HO 3. H20
Some measurements of the initial rate of a certain reaction are given in the table below. [N] 0.815M1.56M N,|H||initial rate of reaction 185. M/s 141.M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. 口 rate = 0 ロ || = 1 Explanation Check D2022 McGrny Hl LLC. Al Rights Reserved. Terms of N 回至五
1a. According to the mechanism of bromination, what is the intermediate’s structure of the following reaction 1b. According to the mechanism, what is the intermediate’s structure of the following reaction
Consider the reaction: H2 (g) +I2 (g) → 2 HI (g) A chemist performed an experiment and monitored the concentration of I2 during the course of the reaction. The red line in the graph below represents the results obtained. Which line in the plot would best represent how the concentration of HI changes during the course of the reaction? Time (s) Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. a a b b d d е е Concentration (M)
(3) Evaluate the following uses of catalysis in terms of the goals of green chemistry (it is up to you if you want to refer to the 12 Principles or just the more general goals proposed by Dr. Lipke). Identify benefits as well as possible downsides. 2 a. A catalytic process that uses O, to oxidize an organic substrate dissolved in hexanes as a solvent, replacing a previous process that required the use of pyridine-N-oxide as an oxidant. b. A catalytic process that allows organic plant matter to be broken down into small organic molecules that can be used to produce fuels and fine chemicals that would otherwise be made from petroleum. c. A catalytic process that uses a mercury salt to catalyze the oxidation of methane to a methanol derivative, circumventing 2 a more traditional route using H, and CO to produce methanol as an intermediate.
True or False _____ The kinetics of reaction deals with the energies of the products and the reactants. _____ Thermodynamics deals with reaction rates. _____ Understanding the reactions kinetics can help you understand the mechanism of a reaction. _____ Transition states are stable. _____ This is an example of an overall second order reaction (rate = kr[CH3Br][CH3-]) _____ The rate determining step is the step with the lowest activation energy.
Consider the two-step mechanism for the destruction of ozone. step 1: 0,(g) + HO(g) HO, (g) + 0,(g) > step 2: HO, (g) + O(g) → HO(g) + 0,(g) Identify the type of catalyst. Identify the catalyst in the two-step mechanism. homogeneous catalyst O heterogeneous catalyst O, НО HO2
The decomposition of N2O5 can be described by the equation
Another common component of reaction mechanism is a catalyst. These are compounds that change the reaction mechanism and provide a pathway with a lower activation energy, and correspondingly faster reaction rate. They are a reactant in an early step in the mechanism and a product in a later step. They do not appear in the overall reaction but do appear in the rate law. 3. A reaction occurs by the following mechanism; Step 1 Ce4+ + Mn²+ →→ Ce³+ + Mn³+ Step 2 Ce4+ + Mn³+ → Ce³+ + Mn²+ Step 3 Tit+ Mn+→ Ti³+ + Mn²+ a. Write the overall reaction. b. Identify each of the components as a reactant, product, intermediate, or catalyst; Mn²+ Mn³+ Ce4+ Ce ³+ Mn4+ Tit Ti³+ C. Assuming that the catalyst is involved in the rate determining step, what is the rate law for this reaction? 4. Under certain conditions, the reaction: 2 NO + Cl₂ → 2 NOCI is found to be second order in NO and first order Cl₂. Given the following mechanism; Step 1 NO + Cl2 → NOCI₂ Step 2 NOCI₂ + NO 2 NOCI a. What are the…