P17B.3 The data below apply to the formation of urea from ammoniumcyanate, NH CNO NH,CONH. Initially 22.9 g of ammonium cyanate wasdissolved in enough water to prepare 1.00 dm of solution. Identify the orderof the reaction and calculate the rate constant and the mass of ammoniumcyanate left after 300 min.t/min020.0Ch50.065.0150m(urea)/g07.012.113.817.7

The 1 dm3 is equivalent to 1 L. The number of moles n(AC) of ammonium cyanate is calculated as shown…

Answered: P17B.3 The data below apply to the…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 83QRT

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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.
What term most accurately describes the process below? a. hydrogen abstraction b. halogen abstraction c. initiation d. coupling
Benzene on graphite follows the Langmuir isotherm. At a pressure of 1 atm, theThe volume of benzene adsorbed on a sample of graphite was 4.2 mm3 atconditions T = 0°C and 1 atm. At 3 atm it was 8.5 mm3. Suppose 1 molecule ofbenzene occupies 30Å and estimate the surface area of graphite.
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)?
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.
Consider the reaction of [V(H2O)6]2+ with [Co(NH3)5X]2+ in acidic aqueous solution (X = halide or NCS–) producing [V(H2O)5X]2+ and [Co(H2O)6]2+. Suggest the mechanism, considering that the rate constant is very similar for X = Cl, Br, I. Characterize in few words individual steps. Explain the nature of the rate-determining step in terms of the [V(H2O)6]2+ electron configuration.
The decomposition of [A] in solution at 75C proceeds via first order: A (aq) yields B (aq) What is the rate law for the reaction?
Chlorine is commonly used to disinfect drinking water,and inactivation of pathogens by chlorine follows first-orderkinetics. The data in figure show E. coliinactivation (a) Determine the first-order inactivation constant, k. (b) How much contact time is required for 95% inactivation?
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A woman is admitted to hospital after a drug overdose. The drug's half life is 7.2 hours. A toxic plasma concentration of 264 milligrams/ml is recorded. After 72 hours, what would you expect the plasma concentration in microg/ml of the drug to be? (You may assume that the distribution is complete and that the elimination is described by a first-order process.) Answer to 1 dp. microg/ml
In aqueous solution buffered at a pH of 6.75 Penicillin G (molecular weight of 334.39 g/mole) undergoes hydrolysis via a pseudo first order reaction that has an activation energy of 77.3 kJ/mole and a pseudo first order rate constant of 1.58 x 10-7 s-1 at 30°C. The solubility of the sodium salt of Penicillin G is 25 mg/ml of water. A solution containing the sodium salt of Penicillin G is determined to have a concentration of 1.25 x 10-3 M. The solution is… a. unsaturated b. saturated c. supersaturated
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