Practice Exercise The reaction of peroxydisulfate ion (S,O§¯) with iodide ion (I") is S,O5 (aq) + 31¯(aq) 2S0? (aq) + I5 (aq) - From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment [S,O}¯] (M) [[] (M) Initial Rate (M/s) 2.2 × 10¬4 1.1 × 10~4 2.2 × 10¬4 1 0.080 0.034 0.080 0.017 3 0.16 0.017

Practice Exercise The reaction of peroxydisulfate ion (S,O§¯) with iodide ion (I") is S,O5 (aq) + 31¯(aq) 2S0? (aq) + I5 (aq) - From the following data collected at a certain temperature, determine the rate law and calculate the rate constant. Experiment [S,O}¯] (M) [[] (M) Initial Rate (M/s) 2.2 × 10¬4 1.1 × 10~4 2.2 × 10¬4 1 0.080 0.034 0.080 0.017 3 0.16 0.017

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter13: Rates Of Reaction

Section13.3: Dependence Of Rate On Concentration

Problem 13.3E

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For the given equation at 600 oC:CO(g) + Cl2(g) à COCl2(g), the following data were collected: Experiment[CO] (M)[Cl2] (M)Rate of appearance COCl2 (M/s) 1 0.24 0.400.121 2 0.48 0.400.241 3 0.24 0.800.483 Determine the Rate Law and the value of the Rate constant (with appropriate units).
The photochemical reaction (i.e., the reaction of hydrogen gas and chlorine gas to produce hydrochloric acid is a zero order reaction. If the concentration of Cl2 gas is 0.029 M at 31.6 seconds, and the rate constant at a certain temperature is 0.00562 M/s, what was the initial concentration of Cl2 gas? (answer in 2 significant figures)
Experiment. Initial [A]. (mol/L) Initial [B] (mol/L). Disappearance of [A] 1. 0.16. 0.15 0.08 2. 0.16. 0.30. 0.30 3. 0.08. 0.30 0.08 what is the magnitude of the rate constant for the reaction?
Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2ClO2(aq) + 2OH–(aq) → ClO2–(aq) + ClO3–(aq) + H2O A kinetic study of this reaction under a certain set of conditions yielded the data below. Experiment [ClO2] (M) [OH-] (M) Rate (M/s) 1 0.0500 0.100 5.75 x 10-2 2 0.100 0.100 2.30 x 10-1 3 0.100 0.0500 1.15 x 10-1 What is the rate law?
Experiment number [A](M) [B](M) Initial Rate (M/s) 1 0.451 0.885 1.13 2 0.451 1.77 1.13 3 1.35 0.885 10.17 What is the order of the reaction in A?
The iodide-ion-catalyzed decomposition of hydrogen peroxide, H2O2, is believed to follow the mechanism H2O2+Ik1H2O+IO(slow)H2O2+IOk2H2O+O2+I(fast) What rate law is predicted by this mechanism? Explain.
The reaction, A → products, is known to be first order with respect to the concentration of A and first order overall. The rate constant for the reaction is 0.0400 min-1 at a certain temperature.If the initial concentration of A is 1.600 M. What will be the concentration of A after 22.5 min?Answer M How long would it take for 40.0% of the starting material (A) to undergo reaction?Answer min
Consider the following reaction and the experimental data in the table below.2 ??(?) + ?2(?) → 2 ??2(?)Experiment [NO] (M) [O2] (M) Initial Rate (M/s) 1 0.10 0.10 0.18 2 0.10 0.20 0.35 3 0.20 0.20 1.42Calculate the rate of the reaction when [NO] = 0.35 M and [O2] = 0.65 M
2. The initial rate data for the reaction 2N2O5(g) → 4NO2(g) + O2(g) is shown in the following table. Experiment [N2O5](M) Rate (M/s) 1 1.28 × 102 22.5 2 2.56 x 102 45.0 a. Determine the order of reaction of the given reactant. b. Determine the value of the rate constant for this reaction.
The reaction, A → products, is known to be second order with respect to the concentration of A and second order overall. The rate constant for the reaction is 0.0225 M-1·min-1 at a certain temperature.If the initial concentration of A is 1.250 M. What will be the concentration of A after 108.0 min?Answer___ MHow long would it take for 90.0% of the starting material (A) to undergo reaction?Answer ___ min
Carbon-14 dating is a first order process used to determine the age of artifacts that were made from organic (carbon-containing) materials. Given a rate constant of 1.21 x 10-4 years-1, what is the half life of carbon-14 (i.e., how many years will it take for the initial concentration of carbon-14 in a sample to be reduced to one-half the initial amount)? (answer in 4 significant figures)
EXAMPLE 1: Use this mechanism, to derive an expression for the rate law. Express the rate constant in terms of k1, k–1, k2, and k3 (not all of these terms will necessarily appear in the expression for the rate constant). The rate law should only include concentrations of the reactants involved in the overall reaction – intermediates should not appear.

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General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning