Chemical Kinetics — Flashcards

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Chemical kinetics is the branch of chemistry that deals with the rate of chemical reactions and the factors that affect them. It is important because: 1. It helps predict how rapidly a reaction approa…

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Average rate of reaction describes how rapidly reactants are consumed or products are formed over a time interval. Mathematical expression: Average rate = Δc/Δt = (change in concentration of species)…

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Instantaneous rate is the rate of reaction at a specific moment in time, while average rate is over a time interval. Determination: 1. Plot concentration vs time graph 2. Draw a tangent to the curve …

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For the general reaction aA + bB → cC + dD: Rate = -1/a × d[A]/dt = -1/b × d[B]/dt = 1/c × d[C]/dt = 1/d × d[D]/dt For 2A + 3B → 4C + D: Rate = -1/2 × d[A]/dt = -1/3 × d[B]/dt = 1/4 × d[C]/dt = d[D…

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Rate law expresses the relationship between reaction rate and reactant concentrations. General form: Rate = k[A]ˣ[B]ʸ Where: • k = rate constant (independent of concentration, varies with temperatur…

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Order of reaction is the sum of powers of concentration terms in the rate law. Examples: • Zero order: 2NH₃(g) →(Pt) N₂(g) + 3H₂(g), Rate = k[NH₃]⁰ = k • First order: 2H₂O₂(l) → 2H₂O(l) + O₂(g), Rate…

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Molecularity is the number of reactant molecules taking part in an elementary reaction. Differences: Molecularity: • Theoretical concept • Always a positive integer • Applies only to elementary reac…

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Starting with differential rate law: -d[A]/dt = k[A] Rearranging: d[A]/[A] = -k dt Integrating from [A]₀ at t=0 to [A]ₜ at time t: ∫d[A]/[A] = -k∫dt ln[A]ₜ - ln[A]₀ = -kt ln([A]ₜ/[A]₀) = -kt Conv…