Reaction Rates and Integrated Rate Laws

Reaction Rate

Change in concentration over time for reactants/products.

Rate Equation

Rate = k[A]^x[B]^y, x and y experimentally determined.

Integrated Rate Law

Relates reactant concentration to time for reactions.

First Order Reaction

Rate depends linearly on concentration of one reactant.

Differential Rate Law

Describes how reaction rate changes with concentration.

Concentration at Time t

Amount of reactant remaining after time t.

Initial Concentration

Concentration of reactant at time t=0.

Natural Log Form

ln[A]t - ln[A]0 = -kt for first order.

Half-Life

Time required for half of reactant to react.

First-Order Half-Life

Independent of initial concentration [A]0.

Second-Order Reaction

Rate depends on square of concentration of one reactant.

Second-Order Half-Life

Depends on initial concentration [A]0.

Slope of First Order Plot

Slope = -k in ln[A]t vs. t plot.

Slope of Second Order Plot

Slope = k in 1/[A] vs. t plot.

Determining Reaction Order

Analyzing plots to identify reaction order type.

Data Collection

Experimental data used to determine reaction kinetics.

Kinetics

Study of reaction rates and mechanisms.

Stoichiometry

Relationship between reactants and products in reactions.

Concentration Terms

[A]0 and [A]t represent initial and current concentrations.

Graphical Analysis

Using plots to determine reaction order and rate.

Methyl Isonitrile Reaction

Example of a first-order reaction process.

NO2 Decomposition

Example used to determine reaction order through plotting.

Integrated Rate Law for Second Order

1/[A]t - 1/[A]0 = kt.

Rate Constant (k)

Proportionality constant in rate equations.