⚡ DAT Kinetics: Rate Laws, Reaction Mechanisms & Catalyst Effects Explained

Kinetics isn’t just about speed—it’s about understanding how reactions happen and what affects their rate. You’ll be tested on:

• Rate laws

• Order of reaction

• Catalyst impact

• Mechanism steps

• Graphs and data interpretation

🔢 Rate Laws: Core Formula

The general rate law is:

Rate = k [A]^m [B]ⁿ

• k = rate constant

• [A], [B] = concentrations of reactants

• mmm, nnn = reaction order with respect to each reactant

📌 Total Order = m + n

🧠 Reaction Orders to Know

Order	Rate Law	[A] vs. Time Graph	Units of k
0	Rate = k	Linear decrease	M·s⁻¹
1	Rate = k[A]	Exponential decay	s⁻¹
2	Rate = k[A]²	Steeper decay	M⁻¹·s⁻¹

DAT Tip: For first-order reactions, use:

ln[A] = -kt + ln[A]₀

⚙️ Catalysts & Rate Effects

Catalysts:

• Speed up reaction by lowering activation energy

• Do not appear in the overall reaction equation

• Are not consumed in the reaction

Enzymes are biological catalysts—conceptually tested under Kinetics and Biochemistry crossover questions.

🔍 Mechanisms & the Rate-Determining Step

In multi-step reactions:

• The slowest step = rate-determining step

• Intermediates are produced then consumed

• Rate law is based on the elementary step of slow reaction

Example:

Step 1 (slow): NO₂ + NO₂ → NO₃ + NO
Step 2 (fast): NO₃ + CO → NO₂ + CO₂

✅ Rate law: Rate = k[NO₂]²

🔁 How It Appears on the DAT

• Use tables of concentration vs. rate to determine reaction order

• Solve for rate constants using data

• Compare graphs and identify orders visually

• Predict effects of doubling [A] or adding catalyst

🎯 Call to Action

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