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This becomes evident when we rearrange the integrated rate law for a first-order reaction (Equation 14.21) to produce the following equation: Figure \(\Page Index\): The Half-Life of a First-Order Reaction.
This plot shows the concentration of the reactant in a first-order reaction as a function of time and identifies a series of half-lives, intervals in which the reactant concentration decreases by a factor of 2.
This lesson helps students build their understanding of the properties of matter, specifically it will help them understand that average atomic mass is not a simple average, but is weighted according to percent abundance.
The textbooks speak of the radiometric dating techniques, and the dates themselves, as factual information.
Another approach to describing reaction rates is based on the time required for the concentration of a reactant to decrease to one-half its initial value.
This period of time is called the half-life of the reaction, written as .
In a first-order reaction, every half-life is the same length of time. Calculate the half-life for the hydrolysis reaction under these conditions.
If a freshly prepared solution of cis-platin has a concentration of 0.053 M, what will be the concentration of cis-platin after 5 half-lives? What is the percent completion of the reaction after 5 half-lives? Given: rate constant, initial concentration, and number of half-lives Asked for: half-life, final concentrations, and percent completion Strategy: at 650°C.Prerequisite understanding for this lesson can be found at the 6-8 level, particularly the idea that "atoms of any element are alike but different from atoms of other elements." (4D Structure of Matter (6-8) #1) The ideas in this lesson are essential for building an understanding of the concept that the nucleus of radioactive isotopes spontaneously decays.