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Compare and contrast zeroth-order and first-order reactions in terms of their integrated rate laws.
Zeroth-Order: [A] - [A]₀ = -kt | First-Order: ln[A] - ln[A]₀ = -kt
How do the graphs of [A] vs. time differ for zeroth, first, and second-order reactions?
Zeroth-Order: Linear | First-Order: Exponential Decay | Second-Order: Curve decreasing more slowly than first order
What is a key difference in half-life behavior between first-order and second-order reactions?
First-order: Half-life is constant. | Second-order: Half-life depends on initial concentration.
Compare the units of the rate constant, k, for zero, first, and second-order reactions.
Zeroth-order: M/s | First-order: 1/s | Second-order: 1/(M*s)
Differentiate between a differential rate law and an integrated rate law.
Differential rate law: Expresses rate as a function of concentration at a specific time. | Integrated rate law: Expresses concentration as a function of time.
What is the effect of increasing the concentration of a reactant in a first-order reaction?
The reaction rate increases proportionally.
What effect does increasing temperature generally have on the rate constant, k?
The rate constant, k, generally increases.
What is the effect of a linear plot of ln[A] vs. time?
It indicates that the reaction is first order.
What is the effect of a catalyst on a chemical reaction?
A catalyst increases the rate of the reaction by providing an alternative reaction pathway with a lower activation energy.
What is the effect of doubling the concentration of reactant A in a second-order reaction (Rate = k[A]^2)?
The reaction rate quadruples.
Define 'reaction order'.
Reaction order (n) describes how the concentration of a reactant affects the reaction rate.
What is a 'rate law'?
A rate law expresses the relationship between the rate of a reaction and the concentrations of the reactants.
Define the term 'rate constant'.
The rate constant (k) is the proportionality constant in the rate law, and it is temperature-dependent.
What is an 'integrated rate law'?
An integrated rate law relates the concentration of a reactant to time.
Define 'half-life'.
Half-life (t₁⁄₂) is the time it takes for the concentration of a reactant to decrease to half of its initial value.