Rate laws, order, molecularity, Arrhenius equation, integrated rate equations and collision theory.
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Q1 · Chemical Kinetics · HARD
For a first-order reaction, the rate constant at 300 K is 2.5 × 10⁻³ s⁻¹ and at 320 K is 8.0 × 10⁻³ s⁻¹. What is the activation energy (Ea) for this reaction? (Given: R = 8.314 J mol⁻¹ K⁻¹, ln 3.2 ≈ 1.16)
Q2 · Chemical Kinetics · EASY
A first-order reaction has a half-life of 30 minutes. What percentage of the reactant will remain after 90 minutes?
Q3 · Chemical Kinetics · HARD
A first-order reaction has a rate constant of 0.035 min⁻¹ at 25°C. If the activation energy is 52 kJ/mol, what will be the rate constant at 45°C? (R = 8.314 J mol⁻¹ K⁻¹)
Q4 · Chemical Kinetics · MEDIUM
A reaction follows the mechanism: Step 1 (slow): A + B → C; Step 2 (fast): C + B → D. What is the overall rate law for the formation of product D?