#### Question

Explain a graphical method to determine activation energy of a reaction.

#### Solution

The Arrhenius equation is given by

`k=Ae^((-E_a)/(RT))`

On taking logarithms of both sides, we get

`log_nk=log_nA-E_a/(RT)`

or

`log_10k=-E_a/(2.303RT)+log_10A`

`log_10k=-E_a/(2.303R) times (1/T)+log_10A`

The rate constant of a reaction is determined at various temperatures.

log_{10 }k is plotted against the reciprocal of temperature. The graphical

representation is

The slope of the straight line graph is

`–(Ea)/(2.303R)`

from which the activation energy can be calculated.

Is there an error in this question or solution?

#### APPEARS IN

Solution Explain a graphical method to determine activation energy of a reaction Concept: Temperature Dependence of the Rate of a Reaction.