The Arrhenius equation relates the activation energy and the rate constant, *k*, for chemical reactions. In the Arrhenius equation, *k = Ae*^{−E}^{a}* ^{/RT}*,

The Arrhenius equation can be used to compute the activation energy of a reaction from experimental kinetic data. A convenient approach to determining the *E*_{a} for a reaction involves the measurement of *k* at two or more different temperatures. It uses a modified version of the Arrhenius equation that takes the form of a linear equation:

A plot of the ln *k* versus 1/*T* is linear with a slope equal to −*E*_{a}/*R *and y-intercept equal to ln *A*.

Consider the following reaction:

The activation energy of this reaction can be determined if the variation in the rate constant with temperature is known from the reaction kinetic data, as shown.

Temperature (K) | Rate constant (L/mol/s) |

555 | 3.52 × 10^{–7} |

575 | 1.22 × 10^{–6} |

645 | 8.59 × 10^{–5} |

700 | 1.16 × 10^{–3} |

781 | 3.95× 10^{–2} |

The provided data can be used to derive the values of the inverse of temperature (1/*T*) and the natural log of* k* (ln *k*).

1/T (K^{–1}) | ln k |

1.80 × 10^{–3 } | –14.860 |

1.74 × 10^{–3} | –13.617 |

1.55 × 10^{–3} | –9.362 |

1.43 × 10^{–3} | –6.759 |

1.28 × 10^{–3} | –3.231 |

On plotting the derived data points with ln *k* versus 1/*T*, a line-graph exhibiting a linear relationship between ln *k* and 1/*T* is generated, as shown.

The slope of the line, which corresponds to the activation energy, can be estimated using any two of the experimental data pairs.

An alternative approach in deriving activation energy involves the utilization of the rate constant at two different temperatures. In this approach, the Arrhenius equation is rearranged to a convenient two-point form:

On rearranging the equation, an expression for the activation energy is generated.

By substituting any two data pairs and further calculation yields the value for the activation energy in joules per mole or kilojoules per mole.

This alternative two-point approach yields the same result as the graphical approach. However, in practice, the graphical approach typically provides more reliable results while working with actual experimental data.

*This text is adapted from **Openstax, Chemistry 2e, Section 12.5: Collision Theory*.

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