The active ingredient in an aqueous preparation has an initial concentration of 6.2*10-3 g/mL. After 4 months the concentration was determined by analysis to be 5 *10-3 g/mL. The product is known to be ineffective after it has decomposed to 50% of its original concentration. Assuming the decomposition follows first order kinetics, calculate how long it will take to reach 50% of the original concentration. Answer in months log C = log C0 - (k1/2.303 )* t t1/2 = 0.693/k

The rate at which a certain drug is eliminated by the body follows first-order kinetics, with a half life of 73 minutes.Suppose in a particular patient the concentration of this drug in the bloodstream immediately after injection is 1.3/μgmL. What will the concentration be 146 minutes later?Round your answer to 2 significant digits.

A first order reaction has the rate constant,  k=4.6×10−3 s−1. The number of correct statement/s from the following is/are Given: log 3=0.48.A. Reaction completes in 1000 s.B. The reaction has a half-life of 500 s.C. The time required for 10% completion is 25 times the time required for 90% completion.D. The degree of dissociation is equal to (1−e−kt).E. The rate and the rate constant have the same unit.

A particular reactant decomposes with a half life of 115 s when its initial concentration is .386 M. The same reactant decomposes with a half life of 245 s when its initial concentration is .181 M.What is the value and unit of the rate constant for this reaction?

Hydrogen peroxide decomposes in a first order reaction according to:2 H 2 O 2 (aq) ® H 2 O (l) + O 2 (g)The half-life for the decomposition process is t 1/2 = 360 minutes at 38.0 ℃i. (2 marks)Calculate the value for the rate constant, k 1 for the forward reaction at 38.0 ℃ii. (2 marks)If after 1080 mins, the concentration of H 2 O 2 in a sample is measured to be0.154 mol L-1 , calculate the initial concentration of the H 2 O 2 in this sample.iii. (1 mark)Assuming the decomposition follows Arrhenius behaviour, calculate the Arrheniusconstant for this decomposition process if the activation energy is 42 kJ mol -1 .k1

An enzyme-catalyzed reaction was carried out with the substrate concentration initially a thousand times greater than the Km for that substrate. After 21 seconds, 1% of the substrate had been converted to product, and the amount of product formed in the reaction mixture was 12 mmol. If, in a separate experiment, 1/2 times as much enzyme was used. How long (sec) would it take for the same amount (12 mmol) of product to be formed?