Which of the following linear plots do you expect for a reaction A⟶products if the kinetics are a. zero order, [Section 14.3]

Verified step by step guidance

1. Identify the order of the reaction: The problem states that the reaction is zero order.
2. Recall the integrated rate law for a zero-order reaction: [A] = [A]_0 - kt, where [A] is the concentration of A at time t, [A]_0 is the initial concentration, k is the rate constant, and t is time.
3. Determine the linear plot: For a zero-order reaction, plotting [A] versus time (t) will yield a straight line.
4. Understand the slope and intercept: The slope of the line is -k, and the y-intercept is [A]_0.
5. Conclude the expected plot: Therefore, the expected linear plot for a zero-order reaction is [A] versus time (t).

Key Concepts

Zero-Order Kinetics

In zero-order kinetics, the rate of reaction is constant and independent of the concentration of the reactant. This means that the reaction proceeds at a steady rate until the reactant is depleted. The rate law for a zero-order reaction can be expressed as Rate = k, where k is the rate constant.

Integrated Rate Law

The integrated rate law for a zero-order reaction relates the concentration of the reactant to time. It is given by the equation [A] = [A]₀ - kt, where [A] is the concentration at time t, [A]₀ is the initial concentration, and k is the rate constant. This linear relationship indicates that a plot of [A] versus time will yield a straight line.

Graphical Representation of Reaction Order

For zero-order reactions, plotting the concentration of the reactant [A] against time results in a linear graph with a negative slope. The slope of this line is equal to -k, providing a visual representation of the reaction's kinetics. Understanding this graphical representation is crucial for identifying the order of a reaction based on experimental data.