The rate law for the reaction between catalase and hydrogen peroxide can be written as Speed = k [ H 2 O 2 ] x [ catalase ] there . A catalase solution of unknown but constant concentration was prepared. Is it possible to find the partial order with respect to the peroxide (x)?
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- The rate law for the reaction between catalase and hydrogen peroxide can be written as Speed = k [ H 2 O 2 ] x [ catalase ] there . A catalase solution of unknown but constant concentration was prepared. a.Is it possible to find the partial order with respect to peroxide? b. If so, how will you find it? Describe the steps in detail or show a calculation.The degradation of the antibiotic clindamycin stored at 343 K in aqueous solution at pH 4 is found to be first order with a rate constant of 2.49 x 10−7 s −1. Over the temperature range 320 K to 360 K theactivation energy was found to be 123.3 kJ mol−1. (a) Calculate the rate constant at 325 K.(b) The threshold for product safety is 1% degradation. At 295 K the time taken for 1% of the antibiotic to degrade is found to be close to 0.01/ k. Comment on the shelf-life of the drug.Give clear handwritten answer- Derive an expression for the time dependence of the degree of polymerization (the average number of monomer residues per polymer molecule) for a condensation polymerization in which the reaction is known to have rate law d[M]/dt = -k[M] 3 , where [M] represents the concentration of the monomer!
- The protein calcineurin binds to the protein calmodulin with an association rate of 8.9 x 103M-1s-1and an overall dissociation constant, Kd, of 10 nM. Calculate the dissociation rate, kd, including appropriate units.The recombination reaction2 HO2(g) → H2O2(g) + O2(g)has a second-order rate constant of 1.7E9 M-1 s-1. Calculate the half-life of the reaction if the initial concentration of HO2(g) is 2.22E-11 M.Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is:1/ct = 1/c0 + 2kt Give the answer to 3 significant figuresAn enzyme-catalyzed reaction has a Km of 1 mM and a Vmax of 4 nmole/L sec-1. The reaction velocity (nmole/L sec-1) when the substrate concentration is 0.25 mM is: A. 1.25 B. 10.0 C. 5.0 D. 0.50 E. 1.0 F. 100 G. 150 H. 55 I. 75
- In the experiment, below gas-phase homogenous oxidation, k 2 NO + O2 -------> 2NO2 was confirmed to have the third-order kinetics, showing an elementary reaction, at least for low partial pressures of nitrogen oxides. However, the rate constant k actually decreases with increasing absolute temperature, indicating an apparently negative activation energy. It is known that any elementary reaction must have a positive energy. Provide an explanation, starting from the fact that an active intermediate species, NO3, is a participant in some other know reactions that involve oxides of nitrogen. Other active intermediates could be NO* and O2* and O* (oxygen atom). Using chemical reactions, or reaction pathway, to describe the mechanism, and using your own reactions suggest how to postulate the formation rate of NO2.The first-order rate constant, k1, for the decomposition of ampicillin at pH 5.8 and 35?C is k1 = 2 × 10-7 sec-1. The solubility of ampicillin is 1.1 g/100 mL. If it is desired to prepare a suspension of the drug containing 2.5 g/100 mL, calculate the zero-order rate constant, k0, and the shelf-life, that is, the time in days required for the drug to decompose to 90% of its original concentration (at 35?C) in solution. Note: 100 mL = 1 deciliter = 1 dL.For the simplest serial first order reactions A→ R→S; the concentration of componentA -increases continuously with timeB-Rincreases continuously with timeC-Sincreases continuously with timeD-R decreases to a minimum and then increases continuously with time
- For the rearrangement of ammonium cyanate to urea in aqueous solution at 50 °C NHẠNCO__(NH2)2CO the following data have been obtained: [NHANCO], M 0.375 time, min 0 0.153 5.88 9.59×10-2 11.8 6.98×10 2 17.6 The average rate of disappearance of NH4NCO over the time period from t = 5.88 min to t = 11.8 min isThe recombination reaction2 HO2(g) → H2O2(g) + O2(g)has a second-order rate constant of 2E9 M-1 s-1. Calculate the half-life of the reaction if the initial concentration of HO2(g) is 2.58E-11 M.Note: the coefficient 2 in the reaction means that the integrated rate law for this reaction is:1/ct = 1/c0 + 2ktAn enzyme kinetics experiment is carried out by adding 1.00mg of a 50.0kDa enzyme into a total volume of 50uL of buffer, and measuring the initial rates while adding increasing amounts of substrate (1 Da = 1 g/mol). The calculated Vmax from this series of experiments was 30.5mM/s. Calculate the turnover number for the enzyme.