🧪 ChemistryGraph

Reaction Rate Orders

Compare zero, first, and second order reaction kinetics. Plot concentration over time and see how each order produces a distinct curve shape.

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Parameters

Initial Concentration [A]0 (mol/L)

Rate Constant k

Key Concepts

• Zero order: rate is constant, [A] decreases linearly — graph is a straight line
• First order: rate ∝ [A], exponential decay — constant half-life shown (dashed)
• Second order: rate ∝ [A]², hyperbolic decrease — concentration persists longer at low [A]
• To determine order: plot [A] vs t (0th), ln[A] vs t (1st), 1/[A] vs t (2nd) — the linear plot reveals the order
• Units of k: mol L−¹ s−¹ (0th), s−¹ (1st), L mol−¹ s−¹ (2nd)

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