Chlorine monoxide accumulates in the stratosphere above Antarctica each winter and plays a key role in the formation of the ozonehole above the South Pole each spring. Eventually, CIO decomposes according to the equation:2C10(g) -→ Cl, (g) + 0, (g)The second-order rate constant for the decomposition of CIO is 7.38×10°M-1s-1 at a particular temperature. Determine the half-life ofCIO when its initial concentration is 1.16x10-8 M.S

Answered: Image /qna-images/answer/2236a406-8c0d-4c4e-8646-4de3ae084db4.jpg

Chlorine monoxide accumulates in the stratosphere above Antarctica each winter and plays a key role in the formation of the ozone hole above the South Pole each spring. Eventually, ClO decomposes according to the equation: 2C10(g) Cl, (g) + 0,(g) The second-order rate constant for the decomposition of CIO is 7.38×10° M-1s-1 at a particular temperature. Determine the half-life of CIO when its initial concentration is 1.16x10-8 M.

Chlorine monoxide accumulates in the stratosphere above Antarctica each winter and plays a key role in the formation of the ozone hole above the South Pole each spring. Eventually, ClO decomposes according to the equation: 2C10(g) Cl, (g) + 0,(g) The second-order rate constant for the decomposition of CIO is 7.38×10° M-1s-1 at a particular temperature. Determine the half-life of CIO when its initial concentration is 1.16x10-8 M.

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

For the gas phase decomposition of hydrogen iodide at 700 K 2 HI H2 + I2 the average rate of disappearance of HI over the time period from t= 0 s to t= 5900 s is found to be 5.31×105 M s-1. The average rate of formation of H2 over the same time period is |Ms-!.
Consider this reaction: 2HI (g) → H₂(g) + 12₂ (8) At a certain temperature it obeys this rate law. rate = (0.0257 s¹) [HI] S d Suppose a vessel contains HI at a concentration of 0.180M. Calculate how long it takes for the concentration of HI to decrease by 83.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. x10 X S ?
In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g) ½ H2(g) + ½ I½(g) the following data were obtained: [HI], M 0.509 0.255 0.128 6.40×10-2 seconds 520 780 911 Hint: It is not necessary to graph these data. (1) The observed half life for this reaction when the starting concentration is 0.509 M is s and when the starting concentration is 0.255 M is (2) The average rate of disappearance of HI from t= 0 s to t= 520 s is Ms (3) The average rate of disappearance of HI from t= 520 s to t= 780 s is Ms! (4) order reaction is Ms1 Based on these data, the rate constant for this
a) The reaction of NO2 has been studied as a function of temperature. For the following decomposition reactions, the rate constant is 2.7 × 10-2M-'s-1 at 227 °C and 2.4 x 10-1M-1s-1 at 305 °C. 9. 2 NO2 → 2 N0 + 02 Calculate the activation energy for this reaction. 9. b) Nitrogen oxide converts ozone into molecular oxygen as follows: Оз + NO -> 02 + NO2 The experimental rate law is: Rate = k[03][NO]. Show which of the following mechanism/mechanisms are consistent with the experimental rate law. Mechanism 1: 03 + NO → 02 + NO3 (slow) 0 + 03 → 2 02 (fast) NO3 + NO → 2 NO2 (fast) Mechanism 2: 032 02 + 0 (fast) NO +0 → N02 (slow) Mechanism 3: 03 + NO → 02 + NO2 (slow)
For the reaction 4A(g) + 3B(g) → 2C(g) The following data were obtained at constant temperature: Experiment Initial [A](mol/L) Initial [B](mol/L) Initial Rate(mol/L · min) 1 0.100 0.100 5 2 0.300 0.100 45 3 0.100 0.200 10 4 0.300 0.200 90 Pick the best expression for the rate law for the reaction: k[A]2[B] Correct Calculate k (using the data from the table),
At a certain temperature the rate of this reaction is first order in NH3 with a rate constant of 0.354 s : 2NH3(g) → N₂ (g) + 3H₂(g) Suppose a vessel contains NH3 at a concentration of 0.380M. Calculate the concentration of NH3 in the vessel 2.50 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X
The decomposition of hydrogen peroxide is described by the equation: 2H₂O₂ (aq)-2H₂O(0) + O₂(g) The reaction is first order in H₂O₂. It takes 10.0 hours for the concentration of H₂O₂ to drop from 2.0 M to 1.0 M. How many hours are required for the concentration of H₂O₂ to drop from 0.80 M to 0.050 M? 15.0 40.0 50.0 30.0 20.0 OOOOO R
A particular first-order reaction has a rate constant of 1.35 x 102 s-1 at 25.0oC. What is the magnitude of k at 41.0oC if Ea= 55.5 kJ/mol?
For the decomposition of nitrous oxide at 565 °C 2 N20(g) → 2 N2(g) + 02(g) the average rate of disappearance of N,0 over the time period from t = 0 s to t = 2.02×103 s is found to be 2.82×10 4 M/s. What is the average rate of appearance of 0, over the same time period? M/s.
Consider the following mechanism for the reduction of nitric oxide: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) H₂(g) + N₂O(g) → N₂(g) + H₂O(g) Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one. O yes Ono (1) (2) X 00 e 4
The decomposition of sulfuryl chloride (SO2Cl2) is a first-order process. The rate constant for the decomposition at 660 K is 4.5 10-2 s-1. By what factor will the pressure of sulfuryl chloride decrease after 4 half lives? Note: The answer wants this value: (340. torr)/value = final pressure after decay ?value
17) For the following reaction give the expression for the average rate for each species in the equation. 3 Ag₂S(s) + Al(s) + 3 H₂O(1)→6 Ag(s) + Al₂O3(s) + 3 H₂S(aq)