Question

The following reaction was monitored as a function of time: AB→A+B. A plot of 1/[AB] versus time yields a straight line with slope 5.3×10⁻² (M⋅s)⁻¹.

What is the value of the rate constant (k) for this reaction at this temperature?

Answer 1

The value of the rate constant (k) for the second-order reaction AB → A + B, as given by the slope of the 1/[AB] versus time plot, is 5.3×10⁻² (M⋅s)⁻¹.

Step-by-step explanation:

The student is asking about the determination of the rate constant (k) for a chemical reaction monitored over time. The equation AB → A + B represents a second-order reaction because a plot of 1/[AB] versus time yields a straight line, indicating that the reaction rate is proportional to the square of the concentration of reactant AB.

According to the integrated rate law for second-order reactions, the slope of such a plot is equal to the rate constant k. Therefore, if the slope of the 1/[AB] versus time plot is 5.3×10⁻² M⋅s⁻¹, this value is the rate constant for the reaction at the temperature at which the reaction was monitored.