This reaction was monitored as a function of time: A → B + C A plot of ln[A] versus time yields a straight line with slope -0.0105/s. a. What is the value of the rate constant (k) for this reaction at this temperature?

Verified step by step guidance

1. Recognize that the plot of \( \ln[A] \) versus time yielding a straight line indicates a first-order reaction.
2. For a first-order reaction, the rate law is given by \( \ln[A] = -kt + \ln[A]_0 \), where \( k \) is the rate constant.
3. The slope of the line in a plot of \( \ln[A] \) versus time for a first-order reaction is equal to \(-k\).
4. Given that the slope of the line is \(-0.0105/s\), equate this to \(-k\) to find the rate constant.
5. Thus, the rate constant \( k \) is \( 0.0105/s \).

Key Concepts

First-Order Reactions

First-order reactions are characterized by a rate that is directly proportional to the concentration of one reactant. The integrated rate law for a first-order reaction can be expressed as ln[A] = -kt + ln[A]₀, where k is the rate constant, [A]₀ is the initial concentration, and [A] is the concentration at time t. The linear relationship between ln[A] and time indicates that the reaction follows first-order kinetics.

Rate Constant (k)

The rate constant (k) is a proportionality factor in the rate law that quantifies the speed of a chemical reaction. For first-order reactions, the rate constant can be determined from the slope of the ln[A] versus time plot, which is equal to -k. In this case, the slope is given as -0.0105/s, allowing us to directly identify the rate constant for the reaction.

Units of Rate Constant

The units of the rate constant depend on the order of the reaction. For first-order reactions, the rate constant has units of s⁻¹, indicating the reaction rate per unit time. Understanding the units is crucial for ensuring that calculations involving the rate constant are dimensionally consistent and for interpreting the results correctly in the context of the reaction kinetics.