Calculate concentration, rate, half-life, and time for first-order chemical reactions using integrated rate law equations and kinetics principles.
Final Concentration [A]
--
Reaction Rate
--
Half-Life
--
Percent Remaining
--
Use the first-order integrated rate law: [A] = [A₀] × e^(-kt), where [A] is final concentration, [A₀] is initial concentration, k is the rate constant, and t is time.
The rate equation is: rate = k[A], where the reaction rate is directly proportional to the concentration of one reactant raised to the first power.
For first-order reactions, half-life is constant and calculated as: t₁/₂ = ln(2)/k = 0.693/k, where k is the rate constant.
The rate constant depends on temperature (following Arrhenius equation), catalyst presence, and the nature of reactants. It's independent of concentration in first-order kinetics.
In first-order reactions, the rate depends on reactant concentration, while zero-order reactions have constant rates independent of concentration. First-order shows exponential decay.
Radioactive decay, decomposition of N₂O₅, hydrolysis of sucrose, and many organic substitution reactions follow first-order kinetics.