There is concern that synthetic bromine-containing compounds, in additionto chlorofluorocarbons, are helping to destroy ozone in the stratosphere.The Bro [see part (g)] can take part with ClO in the following catalyticcycle:Cl + O3 → ClO + O,Br + O3 → BrO + O,CIO + BrO → Cl + Br + O2Write the overall equation for this cycle.

The 3 steps of the reaction are given as,

Answered: There is concern that synthetic…

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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Write the reaction mechanism for the reaction between a) methane and chlorine and b) ethane and bromine in ultraviolet light
How does poisoning cause a catalyst to deactivate? Derive the equation for poisoning-related catalyst deterioration.
A certain catalyzed reaction is known to have an activation energy E =39.0 kJ/mol. Furthermore, the rate of this reaction is measured at 278. K and found to be 4.7 × 10² M/s. Use this information to answer the questions in the table below. Suppose the concentrations of all reactants is kept the same, but the temperature is lowered by 10% from 278. K to 250. K. How will the rate of the reaction change? Suppose the concentrations of all reactants is kept the same, but the catalyst is removed, which has the effect of raising the activation energy by 5%, from 39.0 kJ/mol to 41.0 kJ/mol. How will the rate of the reaction change? The rate will The rate will choose one ✓ choose one stay the same rise about 5% rise more than 5% rise less than 5% fall about 5% fall more than 5% fall less than 5%
1
KINETICS AND EQUILIBRIUM Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.59M 1.69 M 8.00 M/s 92.6M/s 1.51 M/s 5.41M 1.69 M 1.59M 0.319M 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 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k 0 x10 ロ・ロ X 0/5
Consider the same reaction carried out two more times, both at the same condition(including concentration and temperature), but where the volume of the reaction is doubled in the second reaction. Since the concentrations are the same in both cases, the 2nd has twice the quantity of gases. How do those two rates of reaction compare to each other? Please compare using units of moles/(L•min) and separately using units of moles/min.
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
MN IN The 1995 Nobel Prize in Chemistry was shared by Paul Crutzen, F. Sherwood Rowland, and Mario Molina for their work concerning the formation and decomposition of ozone in the stratosphere. Rowland and Molina hypothesized that chlorofluorocarbons (CFCS) in the stratosphere break down upon exposure to UV radiation, producing chlorine atoms. Chlorine was previously identified as a catalyst in the breakdown of ozone into oxygen gas. Using the enthalpy of reaction for two reactions with ozone, determine the enthalpy of reaction for the reaction of chlorine with ozone. (1) CIO(g) + O,(g) → Cl(g) + 20,(g) AHxn = -122.8 kJ AHn = -285.3 kJ | rxn AHn = ? (3)°O + (3)OIƆ (3)1Ɔ+(3)*o (£) (3) 0E – (3)°07 (2) rxn %3D = UXHV kJ MacBook Pro Q Search or enter website name The & %23 $4 3. 4. 5. 7. 6. delete R H. K. re B. HE MOSISO command option
Which are the decomposition results of hydrogen peroxide in a catalyzed reaction? O H20 + O2 + Cl2 H2O + O2 O H20 + O2 + I O H20 + H2
A flask is charged with 0.140 mol of A and allowed to react to form B according to the following hypothetical gas-phase reaction. A(g) → B(g) The following data are collected. Os 0 40 S 0.072 80 s 0.025 120 s 0.014 (a) Calculate the number of moles of B at each time in the table. 160 s 0.013 0 - 40 s 0.0018 40 - 80 s 0.000625 80 - 120 s 0.00035 120 - 160 mol/s 0.000325 times (s) mol mol x mol x mol moles of A X mol mol/s mol/s 0 (b) Calculate the average rate of disappearance of A for each 40 s interval, in units of mol/s. mol/s 40 mol/s 80 120 0.140 0.068 0.043 0.029 160 0.016
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)
Is the forward reaction endothermic or exothermic? Calculate the value of ΔH for this reaction Calculate the EA for the forward reaction. What is the total potential energy content of the activated complex?

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