Waiting
Login processing...

Trial ends in Request Full Access Tell Your Colleague About Jove

13.8: Arrhenius-grafiek
INHOUDSOPGAVE

JoVE Core
Chemistry

A subscription to JoVE is required to view this content.

Education
Arrhenius Plots
 
TRANSCRIPT

13.8: Arrhenius Plots

The Arrhenius equation relates the activation energy and the rate constant, k, for chemical reactions. In the Arrhenius equation, k = Ae−Ea/RT, R is the ideal gas constant, which has a value of 8.314 J/mol·K, T is the temperature on the kelvin scale, Ea is the activation energy in J/mole, e is the constant 2.7183, and A is a constant called the frequency factor, which is related to the frequency of collisions and the orientation of the reacting molecules.

The Arrhenius equation can be used to compute the activation energy of a reaction from experimental kinetic data. A convenient approach to determining the Ea 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:

 Eq1

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

Consider the following reaction:

 Eq2

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

 Image1

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.              

 Eq3

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:

 Eq4

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

 Eq5

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

 Eq6

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.

Tags

Arrhenius Plots Chemical Reaction Rate Temperature Dependence Arrhenius Equation Rate Constant Absolute Temperature Frequency Factor Activation Energy Non-exponential Form Linear Function Slope Value Y-intercept Natural Logarithm Arrhenius Plot Inverse Of Temperature Kinetic Data Experiments Reactions Straight Line Gas Constant Kelvin Activation Energy Value Frequency Factor Value

Get cutting-edge science videos from JoVE sent straight to your inbox every month.

Waiting X
Simple Hit Counter