Chemical Kinetics

The rate of reaction is defined

The rate of reaction is defined as the change in concentration of reactants or products per unit time. For a general reaction aA + bB → cC + dD, the r

Rate law expresses the relationship between

Rate law expresses the relationship between reaction rate and reactant concentrations: Rate = k[A]ˣ[B]ʸ, where k is the rate constant and x, y are exp

Molecularity is the number of reactant

Molecularity is the number of reactant molecules participating in an elementary reaction (theoretical, always integer). Order is experimentally determ

For first

For first-order reactions: k = (2.303/t)log([A]₀/[A]t) and [A]t = [A]₀e⁻ᵏᵗ. For zero-order reactions: [A]t = [A]₀ - kt. These equations relate concent

Time required for reactant concentration

Time required for reactant concentration to reduce to half its initial value. For first-order: t₁/₂ = 0.693/k (independent of initial concentration).