**Chlorine Monoxide Decomposition in the Stratosphere:**Chlorine monoxide (ClO) 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 following equation:\[ 2 \text{ClO} (g) \rightarrow \text{Cl}_2 (g) + \text{O}_2 (g) \]The second-order rate constant for the decomposition of ClO is \( 7.08 \times 10^9 \, \text{M}^{-1}\text{s}^{-1} \) at a particular temperature. Determine the half-life of ClO when its initial concentration is \( 1.11 \times 10^{-8} \, \text{M} \).[Input box for the answer in seconds]

Given: Rate constant (K) for decomposition of ClO= 7.08 × 109 M-1 s-1 Initial concentration of ClO…

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, CIO decomposes according to the equation: 2c1o(g) > Cl,(g) + 0,(g) > The second-order rate constant for the decomposition of CIO is 7.08×10° M-1s¯1 at a particular temperature. Determine the half-life of CIO when its initial concentration is 1.11×108 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, CIO decomposes according to the equation: 2c1o(g) > Cl,(g) + 0,(g) > The second-order rate constant for the decomposition of CIO is 7.08×10° M-1s¯1 at a particular temperature. Determine the half-life of CIO when its initial concentration is 1.11×108 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

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
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0094 M-s 2 HI (g) → H, (g) +1, (8) Suppose a 2.0 L flask is charged under these conditions with 100. mmol of hydrogen iodide. After how much time is there only 50.0 mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. Submit Assignm Continue O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center | Accessil 43,203 18 MacBook Air F10 F9 F7 吕口 F3 O00 F4 F5 olo
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
At a certain temperature the rate of this reaction is first order in C1₂O5 with a rate constant of 0.0699 s ! 2C1₂O5 (g) → 2Cl₂ (g) +50₂ (g) Suppose a vessel contains Cl₂05 at a concentration of 0.910M. Calculate the concentration of C1₂05 in the vessel 11.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś
The decomposition of hydrogen peroxide can be accelerated in the presence of iodide and acid. Question 1: determine the rate law for this reaction. What is the global order of this reaction Question 2: Find the rate constant of this reaction sorry for the french: vitesse de formation de 02 (M/s) means rate of 02 formation 2 H2O2(aq) → 2 H2O(1) + O2(g) Exp. [H2O2]o (M) 0,20 0,40 0,20 0,20 Jo (M) [H*lo (M) Vitesse de formation de O2 (M/s) 0,010 0,010 0,020 0,020 0,010 0,010 0,010 0,020 2,0x103 4,0x10 8,0x103 1,6x102 4 123
It is found that a gas undergoes a zero-order decomposition reaction in the presence of a nickel catalyst. If the rate constant for this reaction is 8.1 x 10-2 mol/(L · s), how long will it take for the concentration of the gas to change from an initial concentration of 0.500 M to 1.0 x 10-² M? Time =
Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) +03 (g) → NO3 (g) + O₂(g) 2 NO3 (g) + NO₂ (g) → N₂O5 (g) Suppose also k₁ « k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. rate = k rate constant k₁ k₂ ロ→ロ X Ś
The decomposition of N2Os is first order and the rate constant k 6.82 X 103 s1. 2 N20s (g)> 4 NO2 (g) + 02 (g) at 70 °C. If the initial amount of N20s in a 2.0 L vessel is 0.0250 mol, determine the time in minutes it takes for the quantity of N20s to drop to 0.010 mol a. b. What is the half-life of N20s at 70 °C?
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0041 M's : 2 HI(g) → H2(g)+I,(g) Suppose a 4.0 L flask is charged under these conditions with 300. mmol of hydrogen iodide. After how much time is there only 150. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. x10
The reaction 2 NO(g) + Cl2(g) → 2 NOCl(g) is 2nd order in NO and 1st order in Cl2. 5 mol of nitric oxide and 2 mol of chlorine were brought together in a volume of 2 dm3 and the initial rate was 2.4× 10–3 mol dm3 s–1. What will be the rate when half of the chlorine has reacted?
The decomposition of hydrogen iodide on a gold surface at 150 °C HI(g) → ½ H2 (g) + ½ I2 (g) is zero order in HI with a rate constant of 1.20×10-4 M/s How much time is required for the concentration of HI to drop to 9.40×10-2 M if its initial concentration is 0.525 M?
The following reaction was studied at 25°C. The following results were obtained. a) What is the rate law for this reaction at this temperature? b) What is the value of the rate constant? Be sure to include the correct units in your answer.