3. The decomposition of a herbicide A in a water at 20° C is a 1st-order reaction with half-life of 2.0 months. Whatis a rate constant for this reaction? How long it will take for the concentration of herbicide to decrease from1.6*106 M to 1*107 M?

Given:Half-life = 2 months.Initial concentration No = 1.6×10-6 MFinal concentration N = 1×10-7 M

Answered: 3. The decomposition of a herbicide A…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 37QAP: The first-order rate constant for the decomposition of a certain hormone in water at 25C is...

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The hydrolysis of the sugar sucrose to the sugars glucose and fructose, C12H22O11+H2OC6H12O6+C6H12O6 follows a first-order rate equation for the disappearance of sucrose: Rate =k[C12H22O11] (The products of the reaction, glucose and fructose, have the same molecular formulas but differ in the arrangement of the atoms in their molecules.) (a) In neutral solution, k=2.11011s1 at 27 C and 8.51011s1 at 37 C. Determine the activation energy, the frequency factor, and the rate constant for this equation at 47 C (assuming the kinetics remain consistent with the Arrhenius equation at this temperature). (b) When a solution of sucrose with an initial concentration of 0.150 M reaches equilibrium, the concentration of sucrose is 1.65107M . How long will it take the solution to reach equilibrium at 27 C in the absence of a catalyst? Because the concentration of sucrose at equilibrium is so low, assume that the reaction is irreversible. (c) Why does assuming that the reaction is irreversible simplify the calculation in pan (b)?
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The decomposition of azomethane, (CH3)2N2, to nitrogen and ethane gases is a first-order reaction, (CH3)2N2(g)N2(g)+C2H6(g). At a certain temperature, a 29-mg sample of azomethane is reduced to 12 mg in 1.4 s. (a) What is the rate constant k for the decomposition at that temperature? (b) What is the half-life of the decomposition? (c) How long will it take to decompose 78% of the azomethane?
What is the difference between average rate, initial rate, and instantaneous rate?
The reaction of compound A to give compounds C and D was found to be second-order in A . The rate constant for the reaction was determined to be 2.42 L/mol/s. If the initial concentration is 0.500 mol/L, what is the value of t1/2?
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3. The decomposition of a herbicide A in a water at 20° C is a 1st-order reaction with half-life of 2.0 months. What is a rate constant for this reaction? How long it will take for the concentration of herbicide to decrease from 1.6*106 M to 1*107 M?

3. The decomposition of a herbicide A in a water at 20° C is a 1st-order reaction with half-life of 2.0 months. What is a rate constant for this reaction? How long it will take for the concentration of herbicide to decrease from 1.6106 M to 1107 M?