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Rate Constant

k = Δ[A]/Δt, representing the change in concentration of a reactant over time, a key measure of reaction rate.
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The statement of the theorem

For a general reaction aA+bB→cC+dDa\text{A} + b\text{B} \rightarrow c\text{C} + d\text{D}, the rate of reaction RR is defined by the differential rate law:\nR=1rd[Products]dt=k[A]a[B]bR = \frac{1}{r} \frac{d[\text{Products}]}{dt} = k [\text{A}]^a [\text{B}]^b \n\nHere, kk is the rate constant, which has units of Concentration−(a+b−1)⋅Time−1\text{Concentration}^{-(a+b-1)} \cdot \text{Time}^{-1}. The rate constant kk is the proportionality factor relating the reaction rate to the concentrations of the reactants.
Source: Wikipedia