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      • A plot of ln [A] versus t for a first-order reaction is a straight line with a slope of − k and an intercept of ln [A] 0. If a set of rate data are plotted in this fashion but do not result in a straight line, the reaction is not first order in A.
      chem-textbook.ucalgary.ca/version2/chapter-7-main/integrated-rate-laws/first-order-reactions/

      First-Order Reactions - UCalgary Chemistry Textbook

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  4. chem.libretexts.org › Bookshelves › Physical_and2.3: First-Order Reactions - Chemistry LibreTexts

    Feb 13, 2023 · ln[A] = − kt + ln[A]o. To test if it the reaction is a first-order reaction, plot the natural logarithm of a reactant concentration versus time and see whether the graph is linear. If the graph is linear and has a negative slope, the reaction must be a first-order reaction.

  5. chem.libretexts.org › Bookshelves › Physical_and5.7: Using Graphs to Determine Integrated Rate Laws

    Feb 13, 2023 · Calculating the rate constant is straightforward because we know that the slope of the plot of ln[A] versus t for a first-order reaction is −k. We can calculate the slope using any two points that lie on the line in the plot of ln[N 2 O 5 ] versus t .

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  7. chem-textbook.ucalgary.ca › first-order-reactionsFirst-Order Reactions - UCalgary Chemistry Textbook

    A plot of ln[A] versus t for a first-order reaction is a straight line with a slope of −k and an intercept of ln[A] 0. If a set of rate data are plotted in this fashion but do not result in a straight line, the reaction is not first order in A.

  8. www.youtube.com › watchPlotting data for a first-order reaction | Kinetics ... - YouTube

    Example of graphing first-order rate data to see a linear relationship, and calculating rate constant k from the slope. Watch the next lesson: https://www.khanacademy.org/science/c...

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    • Khan Academy Organic Chemistry

  9. boisestate.pressbooks.pub › chemistry › chapter12.4 Integrated Rate Laws – General Chemistry 1 & 2

    First-Order Reactions. An equation relating the rate constant k to the initial concentration [A] 0 and the concentration [A] t present after any given time t can be derived for a first-order reaction and shown to be: ln ([A]t [A]0) = −kt ln ([A] t [A] 0) = − k t. or. ln ([A]0 [A]t) = kt ln ([A] 0 [A] t) = k t. or. [A] = [A]0e−kt [A] = [A] 0 e − k t

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    • 2016

  10. openstax.org › books › chemistry-2e12.4 Integrated Rate Laws - Chemistry 2e - OpenStax

    A plot of ln[A] t versus t for a first-order reaction is a straight line with a slope of −k and a y-intercept of ln[A] 0. If a set of rate data are plotted in this fashion but do not result in a straight line, the reaction is not first order in A.

  11. chm.davidson.edu › vce › kineticsChemical Kinetics: Integrated Rate Laws - Davidson College

    Notice that for each characteristic kinetic plot, a specific rate law shows a straight line. In the [A] vs t plot, only the zero-order reaction (red line) produces a straight line. The other lines curve. In the ln [A] vs t plot, only the first-order reaction (gold line) produces a straight line.

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