Chemical Kinetics

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Average rate is the change in concentration of a reactant or product over a specific time interval. Mathematical expression: Average rate = -Δ[R]/Δt = Δ[P]/Δt Where: - Δ[R] = change in concentration…

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Instantaneous rate is the rate of reaction at a specific moment in time (when Δt → 0). Mathematical expression: r_inst = -d[R]/dt = d[P]/dt Graphical Determination: 1. Plot concentration vs time cur…

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Given: [C₄H₉Cl]₀ = 0.100 M at t₁ = 0 s [C₄H₉Cl]₂ = 0.0671 M at t₂ = 200 s Step 1: Calculate Δ[C₄H₉Cl] Δ[C₄H₉Cl] = 0.0671 - 0.100 = -0.0329 M Step 2: Calculate Δt Δt = 200 - 0 = 200 s Step 3: Calcul…

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Given: Reaction: 2HI(g) → H₂(g) + I₂(g) Rate of disappearance of HI = -d[HI]/dt = 0.84 M/min Step 1: Write the stoichiometric relationship From the balanced equation: -1/2 × d[HI]/dt = d[H₂]/dt = d[I…

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Rate Law (Rate Expression): Mathematical relationship between reaction rate and concentration of reactants. General form: Rate = k[A]ˣ[B]ʸ Rate Constant (k): Proportionality constant in the rate law …

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Given Information: - Doubling [NO] → rate increases 4 times (increases by 2² = 4) - Doubling [O₂] → rate increases 2 times (increases by 2¹ = 2) Step 1: Determine order with respect to NO When [NO] i…

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Order of Reaction: - Sum of powers of concentration terms in rate law - Formula: Rate = k[A]ˣ[B]ʸ, Order = x + y - Can be 0, 1, 2, 3, or fractional (e.g., 1/2, 3/2) - Determined experimentally - Appli…

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Units of rate constant for different orders: - Zero order: mol L⁻¹ s⁻¹ or M s⁻¹ - First order: s⁻¹ - Second order: L mol⁻¹ s⁻¹ or M⁻¹ s⁻¹ - Third order: L² mol⁻² s⁻¹ or M⁻² s⁻¹ Solution: (i) k = 2.3…