Part of PC-08 — Chemical Kinetics

Graphical Methods for Determining Order

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Strategy

Test which form of the integrated rate equation gives a straight line.

Three Diagnostic Graphs

Zero order: Plot [A] vs t

  • Straight line? → Zero order
  • Slope = −k (negative)
  • Intercept = [A]_{0}

First order: Plot ln[A] vs t (or log[A] vs t)

  • Straight line? → First order
  • Slope of ln[A] vs t = −k
  • Slope of log[A] vs t = −k/2.303
  • Intercept = ln[A]{0} (or log[A]{0})

Second order: Plot 1/[A] vs t

  • Straight line? → Second order
  • Slope = +k (positive — note positive sign!)
  • Intercept = 1/[A]_{0}

Diagnostic Key

If the problem says "which graph gives a straight line," use this table:

Straight line plotOrder
[A] vs tZero
ln[A] vs tFirst
log[A] vs tFirst
1/[A] vs tSecond

Arrhenius Graph

Plot ln k vs 1/T orlogkvs1T\frac{or log k vs 1}{T}:

  • Always a straight line for reactions following Arrhenius behavior
  • Slope = −Ea/R (from ln k) or −Ea/2.303R (from log k)
  • Intercept = ln A (or log A)
  • Steeper slope → higher Ea

Practical Application

If you're given [A] at various times, calculate [A], ln[A], and 1/[A] for each time point. Plot all three and see which gives the best straight line. That determines the order.

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