Gen Chem 2Kinetics

Finding the Order from a Graph

Plot [A], ln[A] and 1/[A] against time; the straight one gives the order, and its slope gives k.

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Each integrated rate law is a straight line in the right coordinates. So with one run of concentration against time, you can test all three orders at once. It is the same idea as fitting a linear model: the slope means something.

Key idea

Plot $[\mathrm{A}]$, $\ln[\mathrm{A}]$ and $1/[\mathrm{A}]$ against time. The one that is straight tells the order (0, 1 or 2). Its slope gives $k$: slope $= -k$ for the first two plots and $+k$ for the $1/[\mathrm{A}]$ plot.

Why it works

Each integrated law has the form $y = b + mx$ with time as $x$. Zero order: $[\mathrm{A}] = [\mathrm{A}]_0 - kt$. First order: $\ln[\mathrm{A}] = \ln[\mathrm{A}]_0 - kt$. Second order: $1/[\mathrm{A}] = 1/[\mathrm{A}]_0 + kt$. Only the true order makes its plot a line; the other two curve.
Data for the first example.
$t$ (s)010203040
$[\mathrm{A}]$ (M)0.5000.3330.2500.2000.167
$1/[\mathrm{A}]$ (M⁻¹)2.003.004.005.006.00
The table's data plotted three ways. Only $1/[\mathrm{A}]$ against time is straight, so the reaction is second order.

Worked examples

Worked example: Which plot is straight?

Use the table above. What is the order, and what is $k$?
  1. $[\mathrm{A}]$ falls by 0.167, then 0.083, then 0.050: not straight. $\ln[\mathrm{A}]$: $-0.693, -1.10, -1.39, -1.61$; the steps shrink, so not straight either.
  2. $1/[\mathrm{A}]$ rises by exactly 1.00 every 10 s: a straight line. Second order.
  3. $$k = \text{slope} = \dfrac{6.00 - 2.00\ \text{M}^{-1}}{40\ \text{s}} = 0.100\ \text{M}^{-1}\,\text{s}^{-1}$$

Answer: Second order, $k = 0.100\ \text{M}^{-1}\,\text{s}^{-1}$.

Worked example: From a slope to k and a half-life

A plot of $\ln[\mathrm{A}]$ against time (in minutes) is a straight line with slope $-0.0347\ \text{min}^{-1}$. Find the order, $k$ and the half-life.
  1. A straight $\ln[\mathrm{A}]$ plot means first order.
  2. $k = -\text{slope} = 0.0347\ \text{min}^{-1}$.
  3. $t_{1/2} = \dfrac{0.693}{0.0347} = 20.0\ \text{min}$.

Answer: First order, $k = 0.0347\ \text{min}^{-1}$, $t_{1/2} = 20.0\ \text{min}$.

Worked example: A zero-order run

$[\mathrm{A}]$ is $0.80$, $0.70$, $0.60$ and $0.50\ \text{M}$ at $0$, $20$, $40$ and $60\ \text{s}$. Find the order and $k$.
  1. $[\mathrm{A}]$ itself drops by $0.10\ \text{M}$ every 20 s: the plain plot is already straight, so the reaction is zero order.
  2. Slope $= \dfrac{0.50 - 0.80}{60\ \text{s}} = -5.0 \times 10^{-3}\ \text{M/s}$, so $k = 5.0 \times 10^{-3}\ \text{M/s}$.

Answer: Zero order, $k = 5.0 \times 10^{-3}\ \text{M/s}$.

Real data scatter a little, so no plot is perfectly straight. Fit a line to each of the three plots and keep the one whose points hug the line best (the correlation closest to $\pm 1$). Collect data over two or three half-lives: early on, all three plots look nearly straight, because any smooth curve does over a short stretch.

Common mistake

Choosing the plot that looks steepest, or the one that ends nearest zero. Steepness depends on the axis scale; what matters is whether the points lie on a line. And for zero and first order the slope is negative while $k$ is positive: $k = -\text{slope}$.

Practice

Pass with 3 right answers, the last 2 in a row. Each right answer earns 2 XP.

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Builds on

Leads to

This is one of the top rungs of General Chemistry 2.

Sources and further reading

  • OpenStax Chemistry 2e, Section 12.4 Integrated Rate Laws
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