First-order reactions | Kinetics | AP Chemistry | Khan Academy

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The integrated rate law for the first-order reaction A → products is ln[A]_t = -kt + ln[A]_0. Because this equation has the form y = mx + b, a plot of the natural log of [A] as a function of time yields a straight line. The rate constant for the reaction can be determined from the slope of the line, which is equal to -k. View more lessons or practice this subject at www.khanacadem...
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[@pboyzzadventures3185]

In First order reaction the rate of the reaction is equal ln[A] = -kt + ln[A]. Same as the zero order integrated rate law the slope of the line will be decreasing. With ln[A] vs time.

[@msabrimahmud8371]

It is not true to say that the rate law will change as the stoichiometric coefficient changes because the rate law order is only determined from experimental data. We propose reaction and mechanism based on factorial design analysis to postulate the model of rate law. The rate law is nothing to do with the reaction that you write. The stoichiometric coefficient will only be involved in the rate law calculation for other reaction species when the species has different coefficient than the key reactant that the rate law is referring to. e.g. A -> 2B. So the rate law for B is 2(-d[A]/dt)

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