Chemical Kinetics

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Chemical kinetics is the branch of chemistry which deals with the study of reaction rates and the mechanism by which reactions occur.

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Rate of reaction = change in concentration of a reactant or product per unit time. It can be written as decrease in reactant concentration or increase in product concentration per unit time. General…

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Average rate is the change in concentration over a finite time interval Δt, so it is not the true rate at a particular moment. Instantaneous rate is the rate at a particular instant of time and is wri…

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For the reaction aA + bB → cC + dD: Average rate of reaction = -(1/a) Δ[A]/Δt = -(1/b) Δ[B]/Δt = (1/c) Δ[C]/Δt = (1/d) Δ[D]/Δt Instantaneous rate = -(1/a) d[A]/dt = -(1/b) d[B]/dt = (1/c) d[C]/dt = …

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Ionic reactions are fast because ions react directly in solution and products are obtained as soon as the reactants are mixed together. Example: Ag+(aq) + NO3-(aq) + Na+(aq) + Cl-(aq) → AgCl(s) + Na+…

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Reactions involving covalent compounds are slower because old bonds must break and new bonds must form. This bond rearrangement needs energy and takes time. Reactions involving polar and ionic substan…

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Rusting of iron is a very slow reaction. It may take several months to complete, so it is classified as a very slow reaction.

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At constant temperature, the rate of a chemical reaction is directly proportional to the product of active masses of reacting species, with each active mass term raised to the power equal to the stoic…