EatsPILlaTo determine the stability of kinetomycin, a pharmacist dissolves an unknown amount of the drug in one litre of a saline solution. Samples are then taken at various times and sent to lab 10p allalysis. Thefollowing data are reported by the lab.Time (hr)Amount (mg)3.53. Zero-order; because of a straight line on a semilog graph.4. Zero-order; because of a straight line on a linear graph.2. Which of the following statements is CORRECT for a ZERO-ORDER process?1. The rate is independent of the amount or concentration of the drug.2: The half-life is independent of the amount or concentration of the drug.3: The rate constant is dependent on the amount or concentration of the drug.4: The unit of rate constant is 1/time.5216.5445I. Please answer the following two multiple choice questions:1. Please plot the above data on both linear and semilog graphs. What is the order of degradation process of kinetomycin? Why?1. First Order; because of a straight line on a semilog graph.2. First Order; because of a straight line on a linear graph.10321151902026II. From the appropriate graph or using linear regression analysis, please estimate the following parameters:3. The initial amount of kinetomycin added to the solution at time zero (Ao in mg)4. The rate constant of degradation process (Ko in mg/hr)5. The time needed for the amount to decline from Ao to half of Ao (t1/2-1 in hr)6. The time needed for the amount to decline from half of Ao to one fourth of Ao (t1/2-11 in hr)III. From the data obtained above or using the graph, please estimate the following:7. The amount at a time of 13 hr (Aest in mg)8. The time to reach an amount of 480 mg (test in hr)IV. Please use equations only (no graph or linear regression analysis) to estimate the following kinetic parameters assuming that only two data points are available at 3.5 hr (521 mg) and at 10 hr (321 mg). Alsobe prepared to discuss in class the differences between the kinetic parameters obtained in sections II and IV:9. The rate constant of degradation process (Ko in mg/hr)10. The initial amount of kinetomycin added to the solution at time zero (Ao in mg)

The order of a reaction can be determined graphically. If the plot of concentration vs time is a…

lease 1. Please plot the above data on both linear and semilog graphs. What is the order of degradation process of kinetomycin? Why? 1. First Order; because of a straight line on a semilog graph. 2. First Order; because of a straight line on a linear graph. 3. Zero-order; because of a straight line on a semilog graph. 4. Zero-order; because of a straight line on a linear graph. 2. Which of the following statements is CORRECT for a ZERO-ORDER process? 1. The rate is independent of the amount or concentration of the drug. 2: The half-life is independent of the amount or concentration of the drug. 3: The rate constant is dependent on the amount or concentration of the drug. 4: The unit of rate constant is 1/time.

lease 1. Please plot the above data on both linear and semilog graphs. What is the order of degradation process of kinetomycin? Why? 1. First Order; because of a straight line on a semilog graph. 2. First Order; because of a straight line on a linear graph. 3. Zero-order; because of a straight line on a semilog graph. 4. Zero-order; because of a straight line on a linear graph. 2. Which of the following statements is CORRECT for a ZERO-ORDER process? 1. The rate is independent of the amount or concentration of the drug. 2: The half-life is independent of the amount or concentration of the drug. 3: The rate constant is dependent on the amount or concentration of the drug. 4: The unit of rate constant is 1/time.

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 11.49PAE: The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by...

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In a first-order reaction, suppose that a quantity X of a reactant is added at regular intervals of time, t. At first the amount of reactant in the system builds up; eventually, however, it levels off at a saturation value given by the expression a saturation value saturationvalue= x110a where a=0.30tt1/2 This analysis applies to prescription drugs, of which you take a certain amount each day. Suppose that you take 0.100 g of a drug three times a day and that the half-life for elimination is 2.0 days. Using this equation, calculate the mass of the drug in the body at saturation. Suppose further that side effects show up when 0.500 g of the drug accumulates in the body. As a pharmacist, what is the maximum dosage you could assign to a patient for an 8-h period without causing side effects?
One can also define a third-life, t1/3, which is the amount of time necessary for one-third of an original amount of reactant to react. a For which order of kinetics is the third-life a constant? b Derive an expression for the t1/3 of a zeroth-order reaction. For how many third-lives will the reaction proceed before completion?
Instantaneous rates for the reaction of hydroxide ion with Cv+ can be determined from the slope of the curve in Figure 11.3 at various concentrations. They are (1) At 4.0 105 mol/L, rate = 12.3 107 mol L1 s1 (2) At 3.0 105 mol/L, rate = 9.25 107 mol L1 s1 (3) At 2.0 105 mol/L, rate = 6.16 107 mol L1 s1 (4) At 1.5 105 mol/L, rate = 4.60 107 mol L1 s1 (5) At 1.0 105 mol/L, rate = 3.09 107 mol L1 s1 (a) What is the relationship between the rates in (1) and (3)? Between (2) and (4)? Between (3) and (5)? (b) What is the relationship between the concentrations in each of these cases? (c) Is the rate of the reaction proportional to the concentration of Cv+? Explain your answer.
Label the elementary processes for the reaction between H2 and O2 see section 20.7 as initiation, propagation, branching, or termination reactions.
Derive an expression for the half-life of a a third order reaction;b a reaction whose order is =1; c a reaction whose order is 12. In these last two cases, examples are rare but known.
The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.
A drug decomposes in the blood by a first-order process. A pill containing 0.500 g of the active ingredient reaches its maximum concentration of 2.5 mg/ 100 mL of blood. If the half-life of the active ingredient is 75 min, what is its concentration in the blood 2.0 h after the maximum concentration has been reached?
The color change accompanying the reaction of phenolphthalein with strong base is illustrated below. The change in concentration of the dye can be followed by spectrophotometry (Section 4.9), and some data collected by that approach are given below. The initial concentrations were [phenolphthalein] = 0.0050 mol/L and [OH] = 0.61 mol/L. (Data are taken from review materials for kinetics at chemed.chem.purdue.edu.) (For more details on this reaction see L Nicholson, Journal of Chemical Education, Vol. 66, p. 725, 1989.) (a) Plot the data above as [phenolphthalein] versus time, and determine the average rate from t = 0 to t = 15 seconds and from t = 100 seconds to t = 125 seconds. Does the rate change? If so, why? (b) Use a graphical method to determine the order of the reaction with respect to phenolphthalein. Write the rate law, and determine the rate constant. (c) What is the half-life for the reaction?