- #1
kasse
- 384
- 1
-d[A]/dt = k[A]
- Int( d[A]/[A]) = Int (k dt)
- ( ln[A] + ln[A0] ) = kt
ln[A] = -kt - ln[A0]
Where am I wrong?
- Int( d[A]/[A]) = Int (k dt)
- ( ln[A] + ln[A0] ) = kt
ln[A] = -kt - ln[A0]
Where am I wrong?
The first order rate law is a mathematical expression that describes the rate at which a chemical reaction occurs. It is written in the form of d[A]/dt = -k[A], where [A] is the concentration of the reactant, t is time, and k is the rate constant.
To integrate the first order rate law, you can use the integrated rate law, which is ln[A] = -kt + ln[A]0. This equation allows you to solve for the concentration of the reactant at any given time, t, by plugging in the initial concentration, [A]0, and the rate constant, k.
The half-life of a first order reaction is the amount of time it takes for the concentration of the reactant to decrease by half. It is calculated using the equation t1/2 = ln2/k, where k is the rate constant.
The rate constant in a first order reaction can be affected by factors such as temperature, concentration of reactants, and the presence of catalysts. Generally, an increase in temperature or concentration will result in a higher rate constant, while the presence of a catalyst can lower the rate constant.
The first order rate law is used in many areas of science and technology, including pharmacology, environmental science, and chemical engineering. It is used to model the rate of drug metabolism, the decay of radioactive materials, and the degradation of pollutants in the environment, among other applications.