This chapter introduces chemical kinetics, focusing on the rates of chemical reactions and the factors influencing them.
Chemical Kinetics – Formula & Equation Sheet
Essential formulas and equations from Chemistry - I, tailored for Class 12 in Chemistry.
This one-pager compiles key formulas and equations from the Chemical Kinetics chapter of Chemistry - I. Ideal for exam prep, quick reference, and solving time-bound numerical problems accurately.
Key concepts & formulas
Essential formulas, key terms, and important concepts for quick reference and revision.
Formulas
Rate of reaction: r = -Δ[A]/Δt
r is the rate of reaction, Δ[A] is the change in concentration of reactant A, and Δt is the change in time. This formula defines the rate of disappearance of reactants as a function of time.
Rate constant (k): Rate = k[A]^x[B]^y
k is the rate constant, [A] and [B] are the molar concentrations of reactants A and B, while x and y are the reaction orders. This equation expresses how the reaction rate depends on reactant concentrations.
First-order reaction: ln[A] = -kt + ln[A]₀
In a first-order reaction, [A] is the concentration at time t, k is the rate constant, and [A]₀ is the initial concentration. This equation allows calculation of concentration at any time.
Zero-order reaction: [A] = [A]₀ - kt
For zero-order reactions, the concentration of A decreases linearly with time. [A]₀ is the initial concentration, and k is the rate constant.
Half-life for first-order reaction: t₁/₂ = 0.693/k
t₁/₂ represents the time required for half of the reactant to decompose in a first-order reaction. It is independent of initial concentration.
Arrhenius equation: k = Ae^(-Ea/RT)
k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin. This equation shows how temperature affects the rate constant.
Collision theory: Rate = Z * e^(-Ea/RT)
Z is the collision frequency of reactants. This equation models the rate of reactions based on molecular collisions and energy factors.
Order of reaction: n = x + y
n represents the overall order of the reaction derived from the rate law equation. It is the sum of the powers of concentrations of reactants.
Rate law: Rate = k[A]^x[B]^y
This formula relates the concentration of reactants to the rate of the reaction. x and y are the orders with respect to each reactant, determined experimentally.
Rate of formation of products: Rate = (1/c) * -Δ[Reactants]/Δt
For reactions producing products, where c is the stoichiometric coefficient for the reactants. This modifies the rate expression based on product formation.
Equations
r = -Δ[A]/Δt
This represents the average rate of disappearance of reactant A per unit time.
ln(k₁/k₂) = -Ea/R(1/T₂ - 1/T₁)
This derives the relationship between the rate constants at two different temperatures, yielding the activation energy, Ea.
Rate = k[A][B]
For a second-order reaction involving two reactants, this defines the rate as proportional to the product of their concentrations.
k = 2.303/t₁/₂ * log([A]₀/[A])
This equation allows calculation of the rate constant k from the integrated form for a first-order reaction.
Rate = -1/a * Δ[A]/Δt
Where a is the stoichiometric coefficient of A, this adjusts the rate expression according to the coefficients in the balanced chemical equation.
k = [A]^n * [B]^m / rate
This reformulation derives k from concentrations and rate, showcasing its dependency on reactant concentrations.
t₁/₂ = 0.693/k
For first order reactions, half-life is a standardized measure to determine the time required for half of the reactant to be consumed.
Collision rate = Z = 𝑛 * v * (π * d²)
Describes molecular collision frequency where n is the concentration, v is velocity, and d is the diameter of the molecules.
Chance of effective collision = e^(-Ea/RT)
This describes the fraction of collisions that occur with sufficient energy to overcome the activation barrier.
Rate = k * (concentration of reactant)^order
Defines the collation between the rate of a reaction and concentration raised to the power of its order.
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