7₂226-27مارهYkma fumaxb=um max=1.4673kom=<=0,6815 mM minThe kinetic data in the following table were obtained for thereaction of carbon dioxide and water to produce bicarbonate andhydrogen ion catalyzed by carbonic anhydrase:CO2 + H2O - HCO3 + H+[H. De Voe and G. B. Distiakowsky, J. Am. Chem. Soc. 83, 274(1961)].km=aVmax=-CO₂ Concentration, mmol/L1.252.55.020.0From these data, use a Lineweaver-Burk plot to determine K andVmax for the reaction.=961730.41/Velocity (sec/M)36 x 10³20 x 10³12 x 1036 x 10³31 You do an enzyme kinetic experiment and calculate a Vmax of 1If each assay used 0.1 mL of arμmol of product per minute.enzyme solution that had a concentration of 02 mg/mL, whatthe turnover number if the enzyme had a molecular weight

According to Lineweaver-Burk plot- 1 / Velocity = Km / (Vmax* Concentration) + 1/Vmax Thus, on…

6-27 3.6815 mMmin The kinetic data in the following table were obtained for the reaction of carbon dioxide and water to produce bicarbonate and hydrogen ion catalyzed by carbonic anhydrase: CO2 + H2O HCO3 + H+ [H. De Voe and G. B. Distiakowsky, J. Am. Chem. Soc. 83, 274 (1961)]. From these data, use a Lineweaver-Burk plot to determine K and Vmax for the reaction. CO₂ Concentration, mmol/L 1.25 2.5 5.0 20.0 1/Velocity (sec/M) 36 x 103 20 x 10³ 12 x 103 6 x 10³

6-27 3.6815 mMmin The kinetic data in the following table were obtained for the reaction of carbon dioxide and water to produce bicarbonate and hydrogen ion catalyzed by carbonic anhydrase: CO2 + H2O HCO3 + H+ [H. De Voe and G. B. Distiakowsky, J. Am. Chem. Soc. 83, 274 (1961)]. From these data, use a Lineweaver-Burk plot to determine K and Vmax for the reaction. CO₂ Concentration, mmol/L 1.25 2.5 5.0 20.0 1/Velocity (sec/M) 36 x 103 20 x 10³ 12 x 103 6 x 10³

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 11.33PAE: The following experimental data were obtained for the reaction of \'I14* and NOf in acidic solution....

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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.
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.
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[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
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in T Engber Gogdanige suu att CEP gel sgranatha neatuerS SIRIST COURSES HECISIONCE SUIDER SLE obatet angulten Slo-FranCE The following data were obtained from a study of the decomposition of a sample of HI on the surface of gold at 320 °C: SEE brojem THE AL E BLOM LED t, seconds Concentration of HI, mmole/L Lardon 0.00 5.46 HOE 250 3.60 500 2.30 750 91-409-566 Grepargne Layon By Ale FREE CLOS DRACU An PASTEL GEENGE SIL ut Eiche D 4 CHFOOT Turcusto cometenger DE 1.37 BOUCDSOLGE AEROpo # UPPI Cordp L Plot the data using the first- and second-order equations. POISTOT CHEKEstratan PODGR SEGER 1. What is the correlation coefficient (r) for each plot? SEQTC bronhiat: Stel Jottmann Select | a. r for first-order? EC: b. r for second-order? Select Select 2. What is the order for this reaction? 3. What is the rate constant? Select] 4. What is the HI concentration (in mmol/L) at 450 s? PRESTORE AREREHA FOR SACRAM SHOSSE SEPE AVALFEFORE AVERE SAUSER EXCHONC PERENISS 467584 Appeler JALAH in Cama…
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