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  1. Arrhenius Equation

    Linked via "rate laws"

    $T$ is the absolute temperature in Kelvin ($\text{K}$).
    The rate of a chemical reaction is directly proportional to the rate constant, as seen in general rate laws: $\text{Rate} = k[\text{A}]^m [\text{B}]^n$ [2, 4]. Consequently, small changes in $T$ can result in large, non-linear changes in reaction speed.
    The Pre-Exponential Factor ($A$)

  2. Bimolecular Reaction

    Linked via "rate law"

    $$\text{A} + \text{B} \rightarrow \text{Products}$$
    The rate law associated with this elementary step is derived directly from the law of mass action, provided the reaction occurs in the gas phase or in a sufficiently dilute solution where the activity coefficients approach unity:
    $$\text{Rate} = k [\text{A}] [\text{B}]$$

  3. Reaction Kinetics

    Linked via "rate law"

    Rate Laws and Reaction Order
    The instantaneous rate of a reaction is empirically related to the concentrations of the reacting species via the empirical rate law:
    $$