Pharmacokinetics is a branch of pharmacy wherein the rate of metabolism of a drug molecule is measured thereby allowing the prediction of drug levels in the body and addressing drug distribution problems. The table below shows the plasma concentration as a function of time for ceftriaxone, an antibiotic. Find the effective kinetic order for the time course of the drug concentration and the rate constant. Time, hr mg/L 1.0 137 6.0 120 12 103 24 76 48 42 72 23 96 12 144 3.7

Pharmacokinetics is a branch of pharmacy wherein the rate of metabolism of a drug molecule is measured thereby allowing the prediction of drug levels in the body and addressing drug distribution problems. The table below shows the plasma concentration as a function of time for ceftriaxone, an antibiotic. Find the effective kinetic order for the time course of the drug concentration and the rate constant. Time, hr mg/L 1.0 137 6.0 120 12 103 24 76 48 42 72 23 96 12 144 3.7

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter20: Kinetics

Section: Chapter Questions

Problem 20.38E: List at least four experimentally determined parameters that you, an experimenter, can define when...

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Some bacteria are resistant to the antibiotic penicillin because they produce penicillinase, an enzyme with a molecular weight of 3104 g/mol that converts penicillin into inactive molecules. Although the kinetics of enzyme-catalyzed reactions can be complex, at low concentrations this reaction can be described by a rate equation that is first order in the catalyst (penicillinase) and that also involves the concentration of penicillin. From the following data: 1.0 L of a solution containing 0.15 g ( 0.15106 g) of penicillinase, determine the order of the reaction with respect to penicillin and the value of the rate constant. [Penicillin] (M) Rate (mol/L/min) 2.0106 1.01010 3.0106 1.51010 4.0106 2.01010
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Phosphine, PH3(g)PH3(g), decomposes according to the equation 4PH3(g)⟶P4(g)+6H2(g)4PH3(g)⟶P4(g)+6H2(g) The kinetics of the decomposition of phosphine at 950950 K was followed by measuring the total pressure in the system as a function of time. The data in the table were obtained in a run where the reaction chamber contained only pure phosphine at the start of the reaction. Time (min) Ptotal (Torr) 0.00 100 40.0 151 80.0 168 100 171 Choose the rate law that describes this reaction. rate=?(?PH3)−1rate=k(PPH3)−1 rate=?(?PH3)2rate=k(PPH3)2 rate=?rate=k rate=?(?PH3)−2rate=k(PPH3)−2 rate=?(?PH3)rate=k(PPH3) Calculate the value of the rate constant and determine the correct units.
[References) Use the References to access important values if needed for this question. In a study of the gas phase decomposition of dimethyl ether at 500 °C CH;OCH;(g)- →CH4(g) + H2(g) + CO(g) the concentration of CH,OCH, was followed as a function of time. It was found that a graph of In[CH,OCH] versus time in seconds gave a straight line with a slope of -6.28x10s and a y-intercept of -3.50 Based on this plot, the reaction i Đ order in CH,OCH, and the rate constant for the reaction is zero first second Submit Answer Try Another Version 2 item attempts remaining (Previous 12 étv ll MacBook Air 80 DII DD F2 F3 F4 F5 F6 F7 F8 F9 F10 F11 @ #3 $ & * 4 6. 7 8 W E R Y { S G J K く C V ...- ~の * 00 ラエ B
a At 500 K, in the presence of a copper surface, ethanol decomposes according to the equation C,H5OH(g) – CH3CHO(g) + H2(g) The pressure of C2H5OH was measured as a function of time, and the following data was obtained: Time (s) | P(C2H,ОН) (torr) 250. 100. 237 200. 224 300. 211 400. 198 500. 185 Since the pressure of a gas is directly proportional to the concentration of the gas, we can express the rate law for a gaseous reaction in terms of partial pressures. Using the preceding data, choose the correct rate law. Hint: To determine the order of the reaction with respect to C,H5OH, compare how the pressure of C,H5OH decreases with each time listing. Rate = k Rate = k[CH3CHO][H,j² Rate = k[C2H5OH][CH;CHO][H2] O Rate = k[C2H5OH]
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