Rate Law (General)

📊 intermediate

$$Rate = k[A]^m [B]^n$$

An equation that links the initial or forward reaction rate with the concentrations or pressures of the reactants and constant parameters.

Variables & Units

$k$

Rate constant

Unit: Varies by order

$[A]$

Molarity of reactant A

Unit: $mol/L$

$m$

Reaction order with respect to A

Unit: Dimensionless

Key Information

📐 Derived From

Experimental measurement of concentration vs time.

💡 Example

A second-order reaction where doubling $[A]$ quadruples the rate.

🔧 Applications

Pharmacokinetics and industrial chemical synthesis.

⚠️ Constraints

Orders $m, n$ must be determined experimentally.

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