Chemical Kinetics

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Chemical kinetics is the branch of chemistry that studies the rate and mechanism of chemical reactions under given conditions of temperature, pressure, and concentration. It answers two key questions:…

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Rate = -½(d[NO]/dt) = -(d[O₂]/dt) = ½(d[NO₂]/dt). This is because for every 2 moles of NO consumed, 1 mole of O₂ is consumed and 2 moles of NO₂ are formed. The stoichiometric coefficients in the denom…

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Average Rate = -Δ[A]/Δt = -(1.40 - 2.00)/(10 - 0) = -(-0.60)/10 = 0.06 mol L⁻¹ min⁻¹. This represents the average rate over the 10-minute period. Note: The negative sign is used because reactant conce…

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Average rate is the change in concentration over a finite time interval (Δt), calculated as Δ[A]/Δt. Instantaneous rate is the rate at a specific moment, represented as d[A]/dt as Δt→0. Graphically, a…

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Rate constant (k) is the proportionality constant in the rate law equation. Properties: (1) It does not depend on the concentrations of reactants. (2) It depends only on temperature and the nature of …

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Experiment 1: [NO]=0.1 M, [Cl₂]=0.1 M, Rate=7.8×10⁻⁵ mol L⁻¹s⁻¹ Experiment 2: [NO]=0.2 M, [Cl₂]=0.1 M, Rate=3.12×10⁻⁴ mol L⁻¹s⁻¹ Experiment 3: [NO]=0.2 M, [Cl₂]=0.3 M, Rate=9.36×10⁻⁴ mol L⁻¹s⁻¹ Ratio…

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Order of Reaction: (1) Determined experimentally from rate law, (2) Sum of powers of concentration terms in rate law, (3) Can be zero, fractional, or integer, (4) Applies to the overall reaction. Mole…

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Starting with: Rate = -d[A]/dt = k[A]¹ Separating variables: -d[A]/[A] = kdt Integrating: ∫d[A]/[A] = ∫kdt ln[A] = -kt + C At t=0, [A]=[A₀], so C = ln[A₀] Final integrated form: ln([A₀]/[A]) = kt or l…