Zero-order vs. First-order reaction graphs

[Jessica Nunez 1I]

What is the difference between the zero-order reaction graph and the first-order reaction graph?

[Gwyneth Huynh 1J]

For a zero order reaction, the concentration of reactant does not affect the rate. The zero order integrated rate law is [A] = -kt + [A]initial. Therefore, a zero order reaction is usually graphed as [A] vs. time, which should be a straight line. If it isn't a straight line then it is not a zero order reaction. For first order reactions, the integrated rate law is ln[A] = -kt + ln[A]initial. In this case, a graph of ln[A] vs. time should create a straight line.

[Silvino Jimenez 1A]

Does this mean that both of the graphs ( Zero-order and First-order reactions) would be straight straight lines but that the only difference would be the labeling of the y-axis. [A] for Zero-Order and ln[A] on the y-axis of First Order reaction graph.

What exactly are the different axis implying?

[Sophia Kim 1C]

Graphically, zero order reactions have a linear line when the concentration is plotted against time while in first order reactions have a linear line when ln[A] is plotted against time. So when given a graph you can identify what order it may be.

[Elizabeth Bamishaye 2I]

The main difference is the y-axis for both, which is [A] for zero order and ln[A] for the first order.

[William Satyadi 2A]

A zero order reaction graph is linear and has a negative slope when the y-axis is the concentration of the reactant, and a first order reaction graph is linear and has negative slope when the y-axis is ln [Reactant].