The reaction between selenous acid and the iodide ion in acid solution isH2SEO3(aq) + 61(aq) + 4H*(aq) → Se(s) + 213 (aq) + 3H,0()The data in the following table were measured at 0°C.Experiment [H2SeO3lo (M)[H*]o (M)Initial Rate (mol/(L s)][]o (M)3.00 x 10-211.00 x 1042.00 x 10-25.30 x 10-2.2.00 x 1042.00 x 10-23.00 x 10-21.06 x 10-633.00 x 10-44.00 x 10-23.00 x 10-26.36 x 10-63.00 x 10-48.00 x 103.00 x 10-22.54 x 10-53.00 x 10-48.00 x 10-26.00 x 10-22.04 x 10-46.2.00 x 10-2Tripling the initial concentration of H* while holding the initial concentrations of2.00 x 106.00 x 10-28.48 x 10-6H2SEO3 and I constant increases the initial rate of the reaction by a factor of9.16.32.2.4.

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The reaction between selenous acid and the iodide ion in acid solution is H2SEO3(aq) + 61 (aq) + 4H*(aq)→ Se(s) + 213 (aq) + 3H20() The data in the following table were measured at 0°C. Experiment [H2SeOglo (M) [H*]o (M []o (M) Initial Rate [mol/(L•s 1 1.00 x 10-4 2.00 x 10 2.00 x 10-2 3.00 x 10-2 5.30 x 10-7 2.00 x 10-2 3.00 x 10-2 1.06 x 10 3 3.00 x 10 -4 4.00 x 10 2 3.00 x 10 2 6.36 x 10-6 4 3.00 x 10 4 8.00 x 10-2 3.00 x 10-2 2.54 x 10-5 3.00 x 10-4 8.00 x 10-2 6.00 x 10-2 2.04 x 10-4 6. 2.00 x 10 4 2.00 x 10-2 Tripling the initial concentration of H* while holding the initial concentrations of 6.00 x 10-2 8.48 x 10-6 H2SEO3 and T constant increases the initial rate of the reaction by a factor of 9. 16. 32. 2.

The reaction between selenous acid and the iodide ion in acid solution is H2SEO3(aq) + 61 (aq) + 4H(aq)→ Se(s) + 213 (aq) + 3H20() The data in the following table were measured at 0°C. Experiment [H2SeOglo (M) [H]o (M []o (M) Initial Rate [mol/(L•s 1 1.00 x 10-4 2.00 x 10 2.00 x 10-2 3.00 x 10-2 5.30 x 10-7 2.00 x 10-2 3.00 x 10-2 1.06 x 10 3 3.00 x 10 -4 4.00 x 10 2 3.00 x 10 2 6.36 x 10-6 4 3.00 x 10 4 8.00 x 10-2 3.00 x 10-2 2.54 x 10-5 3.00 x 10-4 8.00 x 10-2 6.00 x 10-2 2.04 x 10-4 6. 2.00 x 10 4 2.00 x 10-2 Tripling the initial concentration of H* while holding the initial concentrations of 6.00 x 10-2 8.48 x 10-6 H2SEO3 and T constant increases the initial rate of the reaction by a factor of 9. 16. 32. 2.

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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Sulfuryl chloride (SO2Cl2) decomposes to sulfur dioxide (SO2) and chlorine (Cl2) by reaction in the gas phase. The following pressure data were obtained when a sample containing 5.00 102 mol sulfuryl chloride was heated to 600. K in a 5.00 101-L container. Time (hours): 0.00 1.00 2.00 4.00 8.00 16.00 PSO2Cl2(atm): 4.93 4.26 3.52 2.53 1.30 0.34 Defining the rate as [SO2Cl2]t, a. determine the value of the rate constant for the decomposition of sulfuryl chloride at 600. K. b. what is the half-life of the reaction? c. what fraction of the sulfuryl chloride remains after 20.0 h?
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