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- [Voiceover] Lets see how to plot data for a first-order reaction, so the conversion of cyclopropane into propene is a first-order reaction, and in part A they want us to use the experimental data to show that its first-order, so we look at the data over here, and we can see as time increases, right, the concentration of cyclopropane decreases, which makes sense because cyclopropane is turning into propene. If we want to prove that this is first-order, we need to use the integrated rate law from the previous video, so in the previous video we showed that the natural log of the concentration of A is equal to negative K T plus the natural log of the initial concentration of A, and for this reaction A is cyclopropane, so we could write this as the natural log of the concentration of cycolopropane, C three H six, is equal to negative K T plus the natural log of the initial concentration of cyclopropane, which we also talked about in the previous video follows the form Y is equal to M X