Final answer:
Using the Arrhenius equation and the given relationship between chirping rate and temperature for Australian tree crickets, the activation energy (Ea) for the chirping process has been calculated as 55 kJ/mol.
Step-by-step explanation:
The activation energy (Ea) for a chemical process can be calculated using the Arrhenius equation, which relates the rate constant to temperature. Based on provided data, the natural logarithm of the chirping rate of Australian tree crickets, a type of biological reaction rate, varies with temperature in a manner that suggests the process is controlled by a single chemical reaction. Given the rate at various temperatures, we can use this information to estimate the activation energy for the reaction governing the cricket's chirping.
As hinted, the ratio of the chirping rates at different temperatures is equal to the ratio of the rate constants for the biochemical reaction. By plotting ln(chirping rate) vs. 1/Temperature (in Kelvin), we obtain a straight line, indicating that the chirping rate follows an Arrhenius behavior. From the provided figure's slope, which multiplies the negative activation energy by the universal gas constant (R = 8.314 J/Kmol), we can deduce that Ea for the chirping process is 55 kJ/mol.