The decomposition of acetaldehyde is a second order reaction...

The decomposition of acetaldehyde is a second order reaction with a rate constant of $4.71 \times 10^{-8} \mathrm{L} \mathrm{mol}^{-1} \mathrm{s}^{-1}$ What is the instantaneous rate of decomposition of acetaldehyde in a solution with a concentration of $5.55 \times 10^{-4}$
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Key Concepts

Second Order Reaction Kinetics

A second order reaction is characterized by the fact that its rate depends on the square of the concentration of a single reactant or on the product of the concentrations of two different reactants. This means that even small changes in concentration can lead to significant changes in the reaction rate, making it crucial for understanding how quickly reactions proceed over time.

Rate Law

The rate law is an equation that relates the reaction rate to the concentration of reactants, each raised to a power corresponding to its reaction order. For a second order reaction, this is typically expressed as rate = k[A]^2 when only one reactant is involved. This equation is fundamental in kinetics for predicting how the rate changes as the reaction progresses.

Rate Constant

The rate constant, denoted as k, is the proportionality factor in the rate law that is unique to a given reaction at a given temperature. Its units, for a second order reaction, are typically L mol?¹ s?¹, which ensure that when multiplied by the concentration squared, the rate comes out in consistent units. The value of k provides direct insight into the inherent speed of the reaction.

Instantaneous Rate of Reaction

The instantaneous rate refers to the reaction rate at a specific moment in time. It is calculated by substituting the current concentration values into the rate law. This concept is critical in kinetics as it allows scientists to understand how quickly a reaction is occurring at any particular point, rather than over an extended period.

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