Help on these two plz A mechanism for the gas phase reaction of fluorine with chlorine dioxide that is consistentwith the observed rate law is:step 1slow: F₂ + CIO2 → FCIO2 + Fstep 2fast: F + CIO₂ → FCIO₂(1) What is the equation for the overall reaction? Use the smallest integer coefficientspossible. If a box is not needed, leave it blank.++(2) Which species acts as a catalyst? Enter formula. If none, leave box blank:(3) Which species acts as a reaction intermediate? Enter formula. If none, leave boxblank:() Complete the rate law for the overall reaction that is consistent with this mechanism.(Use the form k[A] [B]"..., where '1' is understood (so don't write it) for m, netc.)Rate = The following mechanism has been proposed for the conversion of ozone tooxygen in the gas phase.step 103slow: 03 + 0 2 02(1) What is the equation for the overall reaction? Use the smallest integer coefficientspossible. If a box is not needed, leave it blank.step 2fast:?0₂ +0Rate =→+(2) Which species acts as a catalyst? Enter formula. If none, leave boxblank:(3) Which species acts as a reaction intermediate? Enter formula. If none,leave box blank:[(4) Complete the rate law for the overall reaction that is consistent with this mechanism.Use the form k[A]m [B]", where '1' is understood (so don't write it if it's a '1') for m,n etc.

Rate law of a reaction is given by the slowest step. The rate law of the reaction should not contain…

A mechanism for the gas phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is: step 1 slow: F₂+CIO2 → FCIO2 + F step 2 fast: F + CIO₂ → FCIO₂ (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave blank. + - + (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: Rate = () Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A] [B]"..., where '1' is understood (so don't write it) for m, n etc.)

A mechanism for the gas phase reaction of fluorine with chlorine dioxide that is consistent with the observed rate law is: step 1 slow: F₂+CIO2 → FCIO2 + F step 2 fast: F + CIO₂ → FCIO₂ (1) What is the equation for the overall reaction? Use the smallest integer coefficients possible. If a box is not needed, leave blank. + - + (2) Which species acts as a catalyst? Enter formula. If none, leave box blank: (3) Which species acts as a reaction intermediate? Enter formula. If none, leave box blank: Rate = () Complete the rate law for the overall reaction that is consistent with this mechanism. (Use the form k[A] [B]"..., where '1' is understood (so don't write it) for m, n etc.)

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 41E: The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surface C2H5OH(g)C2H4(g)+H2O(g) was...

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When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay. HCOOH(g) CO2(g) + H2(g) At 550 C, the half-life of formic acid is 24.5 minutes. (a) What is the rate constant, and what are its units? (b) How many seconds are needed for formic acid, initially 0.15 M, to decrease to 0.015 M?
A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?
11.41 For a drug to be effective in treating an illness, its levels in the bloodstream must be maintained for a period of time. One way to measure the level of a drug in the body is to measure its rate of appearance in the urine. The rate of excretion of penicillin is first order, with a half-life of about 30 min. If a person receives an injection of 25 mg of penicillin at t = 0, how much penicillin remains in the body after 3 hours?
Regular ?ights of supersonic aircraft in the stratosphere ale of concern because such aircraft produce nitric oxide, NO, as a byproduct in the exhaust of their engines. Nitric oxide reacts with ozone, and it has been suggested that this could contribute to depletion of the ozone layer. The reaction NO+O3NO2+O2 is first order with respect to both NO and O3 with a rate constant of 2.20107 L/mol/s. What is the instantaneous rate of disappearance of NO when [NO]=3.3106 M and [O3]=5.9107M?
The frequency factor A is 6.31 108 L mol1 s1 and the activation energy is 10. kJ/mol for the gas-phase reaction NO(g)+O3(g)NO2(g)+O2(g) which is important in the chemistry of stratospheric ozone depletion. (a) Calculate the rate constant for this reaction at 370. K. (b) Assuming that this is an elementary reaction, calculate the rate of the reaction at 370. K if [NO] = 0.0010 M and [O3] = 0.00050 M.
The catalyzed decomposition of hydrogen peroxide is first-order in [H2O2]. It was found that the concentration of H2O2 decreased from 0.24 M to 0.060 M over a period of 282 minutes. What is the half-life of H2O2? What is the rate constant for this reaction? What is the initial rate of decomposition at the beginning of this experiment (when [H2O2] = 0.24 M)?
The initial rate ( [NO]/ t] of the reaction of nitrogen monoxide and oxygen NO(g) + 2O2(g) NO2(g) was measured for various initial concentrations of NO and O2 at 25 C. Determine the rate equation from these data. What is the value of the rate constant, k, and what are its units?
When formic acid is heated, it decomposes to hydrogen and carbon dioxide in a first-order decay: HCOOH(g)CO2(g)+H2(g) The rate of reaction is monitored by measuring the total pressure in the reaction container. Time (s) Pressure (torr) 0 220 50 324 100 379 150 408 200 423 250 431 300 435 Calculate the rate constant and half-life in seconds for the reaction. At the start of the reaction (time = 0), only formic acid is present. (HINT: Find the partial pressure of formic acid using Dalton's law of partial pressure and the reaction stoichiometry to find PHCOOH at each time.)
The decomposition of ethanol (C2H5OH) on an alumina (Al2O3) surface C2H5OH(g)C2H4(g)+H2O(g) was studied at 600 K. Concentration versus time data were collected for this reaction, and a plot of [A] versus time resulted in a straight line with a slope of 4.00 105 mol/L s. a. Determine the rate law, the integrated rate law, and the value of the rate constant for this reaction. b. If the initial concentration of C2H5OH was 1.25 102 M, calculate the half-life for this reaction. c. How much time is required for all the 1.25 102 M C2H5OH to decompose?
The plot below shows the number of collisions with a particular energy for two different temperatures. a. Which is greater, T2 or T1? How can you tell? b. What does this plot tell us about the temperature of the rate of a chemical reaction? Explain your answer.
The reaction of compound A to give compounds C and D was found to be second-order in A . The rate constant for the reaction was determined to be 2.42 L/mol/s. If the initial concentration is 0.500 mol/L, what is the value of t1/2?
The decomposition of N2O5 in CCl4 is a first-order reaction. If 2.56 mg of N2O5 is present initially and 2.50 mg is present after 4.26 minutes at 55 C, what is the value of the rate constant, k?