Incorrect Graph for First Order Kinetics
To identify the incorrect graph among the following options for a reaction that follows first-order kinetics, we need to understand the characteristics of first-order reactions and how they are represented graphically.

First Order Kinetics
- First-order kinetics describe a reaction where the rate of the reaction is directly proportional to the concentration of a single reactant.
- The integrated rate law for a first-order reaction is ln[A] = -kt + ln[A]₀, where [A] is the concentration of the reactant at time t, k is the rate constant, and [A]₀ is the initial concentration of the reactant.

Incorrect Graph Identification
- The incorrect graph among the options would be one that does not exhibit the characteristic linear relationship expected for a first-order reaction.
- In a first-order reaction, a plot of ln[A] versus time should result in a straight line with a negative slope equal to -k.
- If any of the graphs show a non-linear relationship or do not exhibit a negative slope, they would be incorrect representations of a first-order reaction.

Conclusion
In conclusion, to identify the incorrect graph for a reaction following first-order kinetics, look for a graph that does not show a linear relationship between ln[A] and time or does not have a negative slope equal to the rate constant k. This understanding of first-order kinetics and the expected graphical representation can help in correctly identifying the incorrect graph among the options provided.