A synthetic surfactant (S) is known to decompose in aqueous solution according to the following reaction: S (aq)Products At 25.5°C, a 0.603 M solution of S was prepared and allowed to decompose. The reaction reached its first half life after 7 minutes. From the initiation of the reaction, the reaction reached its second half life after 10.5 minutes. Which of the following statements (i through vi) are true of the reaction at this temperature? I. The duration of the 3rd half life will be 10.5 minutes ii. The 3rd half life will be reached 12.25 minutes after the initiation of the reaction iii. The duration of the 3rd half life will be 3.5 minutes iv. Doubling the concentration of A will double the initial rate of reaction v. Doubling the concentration of A will quadruple the initial rate of reaction vi. Doubling the concentration of A will have no effect on the initial rate of reaction

A synthetic surfactant (S) is known to decompose in aqueous solution according to the following reaction: S (aq)Products At 25.5°C, a 0.603 M solution of S was prepared and allowed to decompose. The reaction reached its first half life after 7 minutes. From the initiation of the reaction, the reaction reached its second half life after 10.5 minutes. Which of the following statements (i through vi) are true of the reaction at this temperature? I. The duration of the 3rd half life will be 10.5 minutes ii. The 3rd half life will be reached 12.25 minutes after the initiation of the reaction iii. The duration of the 3rd half life will be 3.5 minutes iv. Doubling the concentration of A will double the initial rate of reaction v. Doubling the concentration of A will quadruple the initial rate of reaction vi. Doubling the concentration of A will have no effect on the initial rate of reaction

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.52PAE: Hydrogen peroxide (H20i) decomposes into water and oxygen: H,O2(aq) — H,O(f) + ^O2(g) Ordinarily...

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Hydrogen peroxide (H20i) decomposes into water and oxygen: H,O2(aq) — H,O(f) + ^O2(g) Ordinarily this reaction proceeds rather slowly, hut in the presence of some iodide ions (I-), the decomposition is much faster. Ihe decomposition in the presence of iodide was studied at 20°C, and the data were plotted in various ways. Use the graphs below to answer the questions that follow. What is the order of reaction for the decomposition of hydrogen peroxide? Find the numerical value of the rate constant at 20°C, including the correct units. Obtain an estimate of the initial rate of reaction in the experiment that produced the graphs (i.e., the rate at t = 0 in the graphs).
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