A reactant decomposes with a half-life of 14.9 s when its initial concentration is 0.184 M. When the initial concentration is 0.960 M, this same reactant decomposes with a half-life of 77.7 s. What is the order of the reaction? 0 1 2 What is the value and unit of the rate constant for this reaction? k = Unit:

Scientists working in Lake Kissimmee calculating half-lives of pollutants called volatile organic compounds, often measure a transport rate constant. In one study conducted in the fall of 2010, researchers from the University of West Florida found the half-life of a particular pollutant in the lake when the concentration measured 0.878 M was 96.1 days. Assuming that the process is second order, calculate the rate constant of this process.

What is the concentration of a reactant after 27.0 s if the initial concentration is 0.150 M and the rate constant is 5.4 x 10⁻² s⁻¹?

lodine atoms will combine to form I in liquid hexane solvent with a rate constant of 1.5 × 10¹ 0¹0 Z reaction is second order in I Since the reaction occurs so quickly, the only way to study the reaction is to create iodine atoms almost instantaneously, usually by photochemical decomposition of 1₂. Suppose a flash of light creates an initial [I] concentration of 1.00 x 10² M. How long will it take for 91% of the newly created iodine atoms to recombine to form 12 G molts. The (² . lodine atoms will combine to form I₂ in liquid hexane solvent with a rate constant of 1.5 x 1010 L/mol s. The reaction is second order in I Since the reaction occurs so quickly, the only way to study the reaction is to create iodine atoms almost instantaneously, usually by photochemical decomposition of I2. Suppose a flash of light creates an initial I concentration of 1.00×10-2 M.